Periodic Trends.ppt for 9th grade chemistry
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Mar 10, 2025
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About This Presentation
periodic grade 9
Slide Content
Periodic Trends
Elemental Properties and Patterns
Elemental Properties and Patterns
Learning
The Periodic Table of Elements
The Periodic Table of Elements
What are Atoms?
• Atoms are the simplest and
smallest particle composed of
protons, electrons, and
neutrons. he number of
•Normally, the number of
protons equals the number of
electrons.
• The number of protons in the
nucleus of an atom is equal to
its atomic number.
The Atom’s Family
• Atoms are the simplest and
smallest particle composed of
protons, electrons, and
neutrons. he number of
•Normally, the number of
protons equals the number of
electrons.
• The number of protons in the
nucleus of an atom is equal to
its atomic number.
The Atom’s Family
Protons, Neutrons and Electrons
•A proton is a positively charged particle
inside the nucleus.
•A neutron is a neutral particle also inside
the nucleus.
•An electron is a negatively charged particle
that orbits the nucleus.
•A proton is a positively charged particle
inside the nucleus.
•A neutron is a neutral particle also inside
the nucleus.
•An electron is a negatively charged particle
that orbits the nucleus.
What is the Periodic Table of
Elements?
• Elements are substances that cannot be
broken down any further by chemical means.
There are over 100!
• The Periodic Table is the arrangement of
these elements by increasing atomic number
and similar properties.
Elements?
• Elements are substances that cannot be
broken down any further by chemical means.
There are over 100!
• The Periodic Table is the arrangement of
these elements by increasing atomic number
and similar properties.
Elements
• Each element on the Periodic Table has an atomic
number, symbol, name and average atomic mass.
• Atomic number – the number of protons found in
the nucleus of an atom.
• Average atomic mass – the mass of an atom
including the protons, neutrons and electrons.
• Each element on the Periodic Table has an atomic
number, symbol, name and average atomic mass.
• Atomic number – the number of protons found in
the nucleus of an atom.
• Average atomic mass – the mass of an atom
including the protons, neutrons and electrons.
How is it Arranged?
•The elements are put into rows by
increasing ATOMIC NUMBER.
•The horizontal rows are called periods and
are labeled 1 to 7.
•The vertical rows are called groups and are
labeled 1 to 18
The red lines show the different periods and the green lines
show the groups.
•The elements are put into rows by
increasing ATOMIC NUMBER.
•The horizontal rows are called periods and
are labeled 1 to 7.
•The vertical rows are called groups and are
labeled 1 to 18
The red lines show the different periods and the green lines
show the groups.
Three States of Matter
Substances are made up of particles.
The state of the substance depends on the arrangement of the particles.
Solid
Particles held tightly
Very close together
Regular arrangement
Vibrate
Can’t move from place
to place
Liquid
Particles held weakly
Very close together
Random arrangement
Vibrate
Constantly move past
each other
Gas
No attraction between
particles
Far apart
Random arrangement
Vibrate
Move quickly in all
directions
The Three States of Matter
Substances are made up of particles.
The state of the substance depends on the arrangement of the particles.
Solid
Particles held tightly
Very close together
Regular arrangement
Vibrate
Can’t move from place
to place
Liquid
Particles held weakly
Very close together
Random arrangement
Vibrate
Constantly move past
each other
Gas
No attraction between
particles
Far apart
Random arrangement
Vibrate
Move quickly in all
directions
The Three States of Matter
Grouped Elements Have Similarities
• Elements in the same group have similar properties.
Remember, groups are columns.
• Chemical Property - a property used to characterize
materials in reactions that change their identity. Ex:
burning something.
• Physical Property - a characteristic of a substance
that can be observed without changing the substance
into something else. Ex: measuring something’s
length, color, mass or volume.
• Elements in the same group have similar properties.
Remember, groups are columns.
• Chemical Property - a property used to characterize
materials in reactions that change their identity. Ex:
burning something.
• Physical Property - a characteristic of a substance
that can be observed without changing the substance
into something else. Ex: measuring something’s
length, color, mass or volume.
Metals, Nonmetals, Metalloids
The Periodic Law
•Dimitri Mendeleev was the first scientist to
publish an organized periodic table of the
known elements.
•He was perpetually in trouble with the
Russian government and the Russian
Orthodox Church, but he was brilliant
never-the-less.
•Dimitri Mendeleev was the first scientist to
publish an organized periodic table of the
known elements.
•He was perpetually in trouble with the
Russian government and the Russian
Orthodox Church, but he was brilliant
never-the-less.
The Periodic Law
•Mendeleev not only predicted the existence
of 2 (at the time) undiscovered elements,
but he predicted the properties too, and he
was right!
•He was very accurate in his predictions,
which led the world to accept his ideas
about periodicity and a logical periodic
table.
•Mendeleev not only predicted the existence
of 2 (at the time) undiscovered elements,
but he predicted the properties too, and he
was right!
•He was very accurate in his predictions,
which led the world to accept his ideas
about periodicity and a logical periodic
table.
The Periodic Law
•Mendeleev
ordered a
periodic table
according to
atomic mass,
which makes
sense (look at a
few in a row)
•Mendeleev
ordered a
periodic table
according to
atomic mass,
which makes
sense (look at a
few in a row)
The Periodic Law
•However this does not work for a 100% of
the elements
•However this does not work for a 100% of
the elements
•In 1913, Henry Moseley decided to arrange
the periodic table by the number of protons,
a.k.a The atomic number
•This is the version that we use today
The Periodic Law
the periodic table by the number of protons,
a.k.a The atomic number
•This is the version that we use today
The Periodic Law
The Periodic Law
•Mendeleev and Moseley understood the
‘Periodic Law’ which states:
•When arranged by increasing atomic number,
the chemical elements display a regular and
repeating pattern of chemical and physical
properties.
•Mendeleev and Moseley understood the
‘Periodic Law’ which states:
•When arranged by increasing atomic number,
the chemical elements display a regular and
repeating pattern of chemical and physical
properties.
The Periodic Law
•Atoms with similar properties appear in
groups or families (vertical columns) on the
periodic table.
•They are similar because they all have the
same number of valence (outer shell)
electrons, which governs their chemical
behavior.
•Atoms with similar properties appear in
groups or families (vertical columns) on the
periodic table.
•They are similar because they all have the
same number of valence (outer shell)
electrons, which governs their chemical
behavior.
Valence Electrons
•Do you remember how to tell the number of
valence electrons for elements in the s- and
p-blocks?
•How many valence electrons will the atoms
in the d-block (transition metals) and the f-
block (inner transition metals) have?
•Most have 2 valence e-, some only have 1.
•Do you remember how to tell the number of
valence electrons for elements in the s- and
p-blocks?
•How many valence electrons will the atoms
in the d-block (transition metals) and the f-
block (inner transition metals) have?
•Most have 2 valence e-, some only have 1.
A Different Type of Grouping
•Besides the 4 blocks (s,p,d,f) of the table,
there is another way of classifying element:
•Metals
•Nonmetals
•Metalloids or Semi-metals.
•Besides the 4 blocks (s,p,d,f) of the table,
there is another way of classifying element:
•Metals
•Nonmetals
•Metalloids or Semi-metals.
Metals, Nonmetals, Metalloids
Metals, Nonmetals, Metalloids
•There is a zig-zag or
staircase line that
divides the table.
•Metals are on the left
of the line, in blue.
•Nonmetals are on the
right of the line, in
orange.
•There is a zig-zag or
staircase line that
divides the table.
•Metals are on the left
of the line, in blue.
•Nonmetals are on the
right of the line, in
orange.
Metals, Nonmetals, Metalloids
•Elements that border
the stair case, shown
in purple are the
metalloids or semi-
metals.
•There is one important
exception.
•Aluminum is a metal
•Elements that border
the stair case, shown
in purple are the
metalloids or semi-
metals.
•There is one important
exception.
•Aluminum is a metal
Metals, Nonmetals, Metalloids
•How can you identify a metal?
•What are its properties?
•What about the less common nonmetals?
•What are their properties?
•And what is a metalloid?
•How can you identify a metal?
•What are its properties?
•What about the less common nonmetals?
•What are their properties?
•And what is a metalloid?
Metals
•Metals are lustrous
(shiny), malleable,
ductile, and are good
conductors of heat and
electricity.
•They are mostly solids
at room temp.
•What is one
exception?
•Metals are lustrous
(shiny), malleable,
ductile, and are good
conductors of heat and
electricity.
•They are mostly solids
at room temp.
•What is one
exception?
Nonmetals
•Nonmetals are the
opposite.
•They are dull, brittle,
nonconductors
(insulators).
•Some are solid, but
many are gases, and
Bromine is a liquid.
•Nonmetals are the
opposite.
•They are dull, brittle,
nonconductors
(insulators).
•Some are solid, but
many are gases, and
Bromine is a liquid.
Metalloids
•Metalloids, aka semi-metals
are just that.
•They have characteristics of
both metals and nonmetals.
•They are shiny but brittle.
•And they are
semiconductors.
•What is our most important
semiconductor?
•Metalloids, aka semi-metals
are just that.
•They have characteristics of
both metals and nonmetals.
•They are shiny but brittle.
•And they are
semiconductors.
•What is our most important
semiconductor?
Alkali Metals
•Elements in Group 1 (not including
Hydrogen).
•Very reactive metals. Always combine
with something else in nature.
•Salt – an Alkali Metal,
Sodium, and another
element, Chlorine,
combined.
•Elements in Group 1 (not including
Hydrogen).
•Very reactive metals. Always combine
with something else in nature.
•Salt – an Alkali Metal,
Sodium, and another
element, Chlorine,
combined.
Alkaline Earth Metals
•Elements in Group 2.
•Reactive Metals that are
always combined with
non-metals in nature.
•Several of these elements
are important mineral
nutrients, like Calcium.
•Elements in Group 2.
•Reactive Metals that are
always combined with
non-metals in nature.
•Several of these elements
are important mineral
nutrients, like Calcium.
Transition Metals
•Elements in Groups 3-12.
•Less reactive, harder metals.
•Includes metals used in jewelry, money and
construction.
•Elements in Groups 3-12.
•Less reactive, harder metals.
•Includes metals used in jewelry, money and
construction.
Boron Family
•Elements in Group 1
•Boron has properties of both metals
and non-metals.
•The rest of the elements in this group
are metals.
•3.
•Elements in Group 1
•Boron has properties of both metals
and non-metals.
•The rest of the elements in this group
are metals.
•3.
Carbon Family
•Elements in Group 14.
•Contains elements important to life and
computers.
•Carbon is the basic element in all organic
compounds.
•Silicon and
Germanium are
important
semiconductors.
•Elements in Group 14.
•Contains elements important to life and
computers.
•Carbon is the basic element in all organic
compounds.
•Silicon and
Germanium are
important
semiconductors.
Nitrogen Family
•Elements in Group 15.
•Nitrogen makes up more than ¾ of our
atmosphere.
•The red tip of matches is made of
phosphorous.
•Elements in Group 15.
•Nitrogen makes up more than ¾ of our
atmosphere.
•The red tip of matches is made of
phosphorous.
Oxygen Family or Chalcogens
•Elements in Group 16.
•Oxygen is necessary for respiration.
•Many things that have a bad odor
contain sulfur.
•Elements in Group 16.
•Oxygen is necessary for respiration.
•Many things that have a bad odor
contain sulfur.
Halogens
•Elements in Group 17.
•Very reactive, diatomic non-metals.
•Always found combined with other
elements in nature.
•Chlorine is used to keep bacteria out of
swimming pools.
•Elements in Group 17.
•Very reactive, diatomic non-metals.
•Always found combined with other
elements in nature.
•Chlorine is used to keep bacteria out of
swimming pools.
Noble Gases
•Elements in Group 18.
•VERY reactive gases.
•Used in lighted neon signs.
•Helium is used to make party balloons float.
•Elements in Group 18.
•VERY reactive gases.
•Used in lighted neon signs.
•Helium is used to make party balloons float.
Elements Used Everyday
Can you think of any elements you use every day?
Can you think of any elements you use every day?
Periodic Trends
•There are several important atomic
characteristics that show predictable trends
that you should know.
•The first and most important is atomic
radius.
•Radius is the distance from the center of the
nucleus to the “edge” of the electron cloud.
•There are several important atomic
characteristics that show predictable trends
that you should know.
•The first and most important is atomic
radius.
•Radius is the distance from the center of the
nucleus to the “edge” of the electron cloud.
Atomic Radius
•Since a cloud’s edge is difficult to define,
scientists use define covalent radius, or half
the distance between the nuclei of 2 bonded
atoms.
•Atomic radii are usually measured in
picometers (pm) or angstroms (Å). An
angstrom is 1 x 10
-10
m.
•Since a cloud’s edge is difficult to define,
scientists use define covalent radius, or half
the distance between the nuclei of 2 bonded
atoms.
•Atomic radii are usually measured in
picometers (pm) or angstroms (Å). An
angstrom is 1 x 10
-10
m.
Covalent Radius
•Two Br atoms bonded together are 2.86
angstroms apart. So, the radius of each
atom is 1.43 Å.
2.86 Å
1.43 Å 1.43 Å
•Two Br atoms bonded together are 2.86
angstroms apart. So, the radius of each
atom is 1.43 Å.
2.86 Å
1.43 Å 1.43 Å
Atomic Radius
•The trend for atomic radius in a vertical
column is to go from smaller at the top to
larger at the bottom of the family.
•Why?
•With each step down the family, we add an
entirely new energy level to the electron
cloud, making the atoms larger with each
step.
•The trend for atomic radius in a vertical
column is to go from smaller at the top to
larger at the bottom of the family.
•Why?
•With each step down the family, we add an
entirely new energy level to the electron
cloud, making the atoms larger with each
step.
Atomic Radius
•The trend across a horizontal period is less
obvious.
•What happens to atomic structure as we
step from left to right?
•Each step adds a proton and an electron
(and 1 or 2 neutrons).
•Electrons are added to existing sublevels.
(They are not getting bigger)
•The trend across a horizontal period is less
obvious.
•What happens to atomic structure as we
step from left to right?
•Each step adds a proton and an electron
(and 1 or 2 neutrons).
•Electrons are added to existing sublevels.
(They are not getting bigger)
Atomic Radius
•The effect is that the more positive nucleus
has a greater pull on the electron cloud.
•The nucleus is more positive and the
electron cloud is more negative.
•The increased attraction pulls the cloud
in, making atoms smaller as we move from
left to right across a period.
•The effect is that the more positive nucleus
has a greater pull on the electron cloud.
•The nucleus is more positive and the
electron cloud is more negative.
•The increased attraction pulls the cloud
in, making atoms smaller as we move from
left to right across a period.
Effective Nuclear Charge
•We call this effect…
•Effective nuclear charge is the pull that an
electron “feels” from the nucleus.
•The closer an electron is to the nucleus, the
more pull it feels.
•As effective nuclear charge increases, the
electron cloud is pulled in tighter.
•We call this effect…
•Effective nuclear charge is the pull that an
electron “feels” from the nucleus.
•The closer an electron is to the nucleus, the
more pull it feels.
•As effective nuclear charge increases, the
electron cloud is pulled in tighter.
Atomic Radius
•Here is an animation to explain the trend.
•It might help to draw arrows like this:
•Here is an animation to explain the trend.
•It might help to draw arrows like this:
Practice…
1.Explain why a magnesium atom is smaller
than atoms of both sodium and calcium
2. Which effect on atomic size is more
significant, an increase in nuclear charge
across a period or an increase in occupied
energy levels within a group? Explain.
1.Explain why a magnesium atom is smaller
than atoms of both sodium and calcium
2. Which effect on atomic size is more
significant, an increase in nuclear charge
across a period or an increase in occupied
energy levels within a group? Explain.
Ionization Energy
•This is the second important periodic trend.
•If an electron is given enough energy to
overcome the effective nuclear charge
holding the electron in the cloud, it can
leave the atom completely.
•The atom has been “ionized” or charged.
•The number of protons and electrons is no
longer equal.
•This is the second important periodic trend.
•If an electron is given enough energy to
overcome the effective nuclear charge
holding the electron in the cloud, it can
leave the atom completely.
•The atom has been “ionized” or charged.
•The number of protons and electrons is no
longer equal.
Ionization Energy
•The energy required to remove an electron
from an atom is ionization energy. (measured
in kilojoules, kJ)
•The larger the atom is, the easier its electrons
are to remove.
•Ionization energy and atomic radius are
inversely proportional.
•The energy required to remove an electron
from an atom is ionization energy. (measured
in kilojoules, kJ)
•The larger the atom is, the easier its electrons
are to remove.
•Ionization energy and atomic radius are
inversely proportional.
Ionization Energy
Ionization Energy (Potential)
Ionization Energy
•If an atom as a low ionization energy, will it
be easy or hard to remove an electron?
•Think about the energy required to remove it, is it
high or low? Do you have to put a large amount of
energy into it or a small amount?
•What if the atom has a high ionization
energy?
•If an atom as a low ionization energy, will it
be easy or hard to remove an electron?
•Think about the energy required to remove it, is it
high or low? Do you have to put a large amount of
energy into it or a small amount?
•What if the atom has a high ionization
energy?
Practice…
1.Compare the first ionization energy of
sodium to that of potassium.
2.Compare the first ionization energy
lithium to that of beryllium.
1.Compare the first ionization energy of
sodium to that of potassium.
2.Compare the first ionization energy
lithium to that of beryllium.
Metallic Character
•This is simple a relative measure of how
easily atoms lose or give up electrons.
•Your help sheet should look like this:
Which
element is
most
metallic?
•This is simple a relative measure of how
easily atoms lose or give up electrons.
•Your help sheet should look like this:
Which
element is
most
metallic?
Electronegativity
•Electronegativity is a measure of an atom’s
attraction for another atom’s electrons.
•It is an arbitrary scale that ranges from 0 to 4.
•Generally, metals are electron donators and
have low electronegativities.
•Nonmetals are electron takers and have high
electronegativities.
•What about the noble gases?
•Do they need anyany electrons?
•Electronegativity is a measure of an atom’s
attraction for another atom’s electrons.
•It is an arbitrary scale that ranges from 0 to 4.
•Generally, metals are electron donators and
have low electronegativities.
•Nonmetals are electron takers and have high
electronegativities.
•What about the noble gases?
•Do they need anyany electrons?
Electronegativity
0
0
Electronegativity
•What is the most electronegative atom?
•Why?
•Fluorine
•It has a small atomic radius, and a high (relative)
effective nuclear charge
•What is the most electronegative atom?
•Why?
•Fluorine
•It has a small atomic radius, and a high (relative)
effective nuclear charge
Practice…
1.Is the electronegativity of barium larger or
smaller than that of strontium? Explain.
2.Arrange oxygen, fluorine, and sulfur in
order of increasing electronegativity.
1.Is the electronegativity of barium larger or
smaller than that of strontium? Explain.
2.Arrange oxygen, fluorine, and sulfur in
order of increasing electronegativity.
Overall Reactivity
•This ties all the previous trends together in
one package.
•However, we must treat metals and nonmetals
separately, as one will gain electrons and one
will lose electrons.
•The most reactive metals are the largest since
they are the best electron givers.
•The most reactive nonmetals are the smallest
ones, the best electron takers.
•This ties all the previous trends together in
one package.
•However, we must treat metals and nonmetals
separately, as one will gain electrons and one
will lose electrons.
•The most reactive metals are the largest since
they are the best electron givers.
•The most reactive nonmetals are the smallest
ones, the best electron takers.
Overall Reactivity
•Think corners
0
•Think corners
0
Overall Reactivity
•Take out a piece of scrap paper or just find a
spot in your notes…
•We are going to watch a video that will react
sodium, potassium, rubidium, and cesium
with water.
•Prediction: Order the 4 elements from least
reactive to most reactive.
•Justify your reasoning!
•Take out a piece of scrap paper or just find a
spot in your notes…
•We are going to watch a video that will react
sodium, potassium, rubidium, and cesium
with water.
•Prediction: Order the 4 elements from least
reactive to most reactive.
•Justify your reasoning!
Alkali metal video
•Extra link (slow motion): http://www.youtube.com/watch?v=iP6CRZdDu6o
•Extra link (slow motion): http://www.youtube.com/watch?v=iP6CRZdDu6o
Ionic Radius
•Cations are always smaller than the original
atom.
•The entire outer PEL is removed during
ionization.
•Conversely, anions are always larger than
the original atom.
•Electrons are added to the outer PEL.
•Cations are always smaller than the original
atom.
•The entire outer PEL is removed during
ionization.
•Conversely, anions are always larger than
the original atom.
•Electrons are added to the outer PEL.
Cation Formation
11p+
Na atom
1 valence electron
Valence e-
lost in ion
formation
Effective nuclear
charge on remaining
electrons increases.
Remaining e- are
pulled in closer to
the nucleus. Ionic
size decreases.
Result: a smaller
sodium cation, Na
+
11p+
Na atom
1 valence electron
Valence e-
lost in ion
formation
Effective nuclear
charge on remaining
electrons increases.
Remaining e- are
pulled in closer to
the nucleus. Ionic
size decreases.
Result: a smaller
sodium cation, Na
+
Anion Formation
17p+
Chlorine
atom with 7
valence e-
One e- is added
to the outer
shell.
Effective nuclear charge is
reduced and the e- cloud
expands.
A chloride ion is
produced. It is
larger than the
original atom.
17p+
Chlorine
atom with 7
valence e-
One e- is added
to the outer
shell.
Effective nuclear charge is
reduced and the e- cloud
expands.
A chloride ion is
produced. It is
larger than the
original atom.
Practice…
1.Explain why the sulfide ion (S
-2
) is larger
than the chloride ion (Cl
-
).
2. Would you expect a S
-2
ion to be larger or
smaller than an K
+
ion? Explain.
1.Explain why the sulfide ion (S
-2
) is larger
than the chloride ion (Cl
-
).
2. Would you expect a S
-2
ion to be larger or
smaller than an K
+
ion? Explain.
Apply…
•Would you expect a Cl
-
ion to be larger or
smaller than an Mg
+2
ion? Explain.
•Would you expect a Cl
-
ion to be larger or
smaller than an Mg
+2
ion? Explain.
•Which of the following statements about the periodic table is true?
•a) Elements in the same group have similar chemical properties. ✅
•b) Elements in the same period have the same number of valence electrons.
•c) The atomic number increases from right to left in each period.
•d) Groups are horizontal rows in the periodic table.
•Which of the following is an accurate way to identify a noble gas in the
periodic table?
•a) It has 1 electron in its outermost shell.
•b) It has 8 electrons in its outermost shell. ✅
•c) It has a very high electronegativity.
•d) It is always in the second period.
•In which block of the periodic table would you find the element with the
electron configuration [Ne]3s²3p²?
•a) s-block
•b) p-block ✅
•c) d-block
•d) f-block
•a) Elements in the same group have similar chemical properties. ✅
•b) Elements in the same period have the same number of valence electrons.
•c) The atomic number increases from right to left in each period.
•d) Groups are horizontal rows in the periodic table.
•Which of the following is an accurate way to identify a noble gas in the
periodic table?
•a) It has 1 electron in its outermost shell.
•b) It has 8 electrons in its outermost shell. ✅
•c) It has a very high electronegativity.
•d) It is always in the second period.
•In which block of the periodic table would you find the element with the
electron configuration [Ne]3s²3p²?
•a) s-block
•b) p-block ✅
•c) d-block
•d) f-block
•Which of the following is a characteristic of elements in
the same group of the periodic table?
•a) They have the same atomic number.
•b) They have the same electron configuration in their
outermost shell. ✅
•c) They have identical physical properties.
•d) They form similar types of bonds with other elements
the same group of the periodic table?
•a) They have the same atomic number.
•b) They have the same electron configuration in their
outermost shell. ✅
•c) They have identical physical properties.
•d) They form similar types of bonds with other elements
•Which of the following is the most likely
property of an element found in Group 17
(halogens)?
•a) It has a low ionization energy.
•b) It readily loses electrons to form cations.
•c) It readily gains electrons to form anions. ✅
•d) It has high metallic character.
property of an element found in Group 17
(halogens)?
•a) It has a low ionization energy.
•b) It readily loses electrons to form cations.
•c) It readily gains electrons to form anions. ✅
•d) It has high metallic character.
•Which of the following trends in atomic
radius is observed as you move across a
period from left to right?
•a) Atomic radius increases.
•b) Atomic radius decreases. ✅
•c) Atomic radius remains the same.
•d) Atomic radius first increases then decreases.
radius is observed as you move across a
period from left to right?
•a) Atomic radius increases.
•b) Atomic radius decreases. ✅
•c) Atomic radius remains the same.
•d) Atomic radius first increases then decreases.
•Why does the atomic radius decrease across
a period from left to right?
•a) The number of electron shells increases.
•b) Electrons are added to higher energy levels.
•c) Effective nuclear charge increases, pulling
electrons closer. ✅
•d) Electrons are lost, reducing the size.
a period from left to right?
•a) The number of electron shells increases.
•b) Electrons are added to higher energy levels.
•c) Effective nuclear charge increases, pulling
electrons closer. ✅
•d) Electrons are lost, reducing the size.
•Which element has the largest atomic
radius?
•a) Sodium (Na) ✅
•b) Chlorine (Cl)
•c) Neon (Ne)
•d) Lithium (Li)
radius?
•a) Sodium (Na) ✅
•b) Chlorine (Cl)
•c) Neon (Ne)
•d) Lithium (Li)
•What happens to the atomic radius as
you move down a group in the periodic
table?
•a) It increases. ✅
•b) It decreases.
•c) It stays the same.
•d) It fluctuates.
you move down a group in the periodic
table?
•a) It increases. ✅
•b) It decreases.
•c) It stays the same.
•d) It fluctuates.
•Ionization energy tends to increase as you
move across a period from left to right. What
is the primary reason for this trend?
•a) Electrons become easier to remove.
•b) The nucleus attracts electrons more strongly.
✅
•c) The number of electron shells increases.
•d) The atomic radius increases.
move across a period from left to right. What
is the primary reason for this trend?
•a) Electrons become easier to remove.
•b) The nucleus attracts electrons more strongly.
✅
•c) The number of electron shells increases.
•d) The atomic radius increases.
•Which of the following elements would
have the highest ionization energy?
•a) Potassium (K)
•b) Calcium (Ca)
•c) Neon (Ne) ✅
•d) Magnesium (Mg)
have the highest ionization energy?
•a) Potassium (K)
•b) Calcium (Ca)
•c) Neon (Ne) ✅
•d) Magnesium (Mg)
•What happens to the first ionization
energy as you move down a group in the
periodic table?
•a) It increases.
•b) It decreases. ✅
•c) It remains constant.
•d) It fluctuates significantly.
energy as you move down a group in the
periodic table?
•a) It increases.
•b) It decreases. ✅
•c) It remains constant.
•d) It fluctuates significantly.
•Which of the following is a correct statement
about ionization energy?
•a) Noble gases have the lowest ionization energy.
•b) Alkali metals have the highest ionization energy.
•c) Ionization energy decreases as you move from
left to right across a period.
•d) Ionization energy increases as the number of
protons increases in a period. ✅
about ionization energy?
•a) Noble gases have the lowest ionization energy.
•b) Alkali metals have the highest ionization energy.
•c) Ionization energy decreases as you move from
left to right across a period.
•d) Ionization energy increases as the number of
protons increases in a period. ✅
•Which element has the highest electron
affinity?
•a) Sodium (Na)
•b) Chlorine (Cl) ✅
•c) Oxygen (O)
•d) Argon (Ar)
affinity?
•a) Sodium (Na)
•b) Chlorine (Cl) ✅
•c) Oxygen (O)
•d) Argon (Ar)
•What is electron affinity?
•a) The energy required to add an electron to a
neutral atom. ✅
•b) The energy released when an electron is
removed from an atom.
•c) The tendency of an atom to lose an electron.
•d) The energy released when an atom bonds
with another atom.
•a) The energy required to add an electron to a
neutral atom. ✅
•b) The energy released when an electron is
removed from an atom.
•c) The tendency of an atom to lose an electron.
•d) The energy released when an atom bonds
with another atom.
•Why do halogens have high electron
affinities?
•a) They have a full valence shell.
•b) They easily gain electrons to achieve a
stable configuration. ✅
•c) They tend to lose electrons in reactions.
•d) Their atomic radius is very large.
affinities?
•a) They have a full valence shell.
•b) They easily gain electrons to achieve a
stable configuration. ✅
•c) They tend to lose electrons in reactions.
•d) Their atomic radius is very large.
•Which element has the highest
electronegativity?
•a) Oxygen (O)
•b) Fluorine (F) ✅
•c) Chlorine (Cl)
•d) Nitrogen (N)
electronegativity?
•a) Oxygen (O)
•b) Fluorine (F) ✅
•c) Chlorine (Cl)
•d) Nitrogen (N)
•What happens to electronegativity as you
move from left to right across a period?
•a) Electronegativity increases. ✅
•b) Electronegativity decreases.
•c) Electronegativity remains the same.
•d) Electronegativity fluctuates.
move from left to right across a period?
•a) Electronegativity increases. ✅
•b) Electronegativity decreases.
•c) Electronegativity remains the same.
•d) Electronegativity fluctuates.
•Which of the following elements has the
lowest electronegativity?
•a) Francium (Fr) ✅
•b) Lithium (Li)
•c) Fluorine (F)
•d) Oxygen (O)
lowest electronegativity?
•a) Francium (Fr) ✅
•b) Lithium (Li)
•c) Fluorine (F)
•d) Oxygen (O)
•What is the trend of electronegativity as
you move down a group in the periodic
table?
•a) It increases.
•b) It decreases. ✅
•c) It remains constant.
•d) It fluctuates.
you move down a group in the periodic
table?
•a) It increases.
•b) It decreases. ✅
•c) It remains constant.
•d) It fluctuates.
•Which of the following elements exhibits
metallic character?
•a) Carbon (C)
•b) Sodium (Na) ✅
•c) Sulfur (S)
•d) Oxygen (O)
metallic character?
•a) Carbon (C)
•b) Sodium (Na) ✅
•c) Sulfur (S)
•d) Oxygen (O)
•As you move across a period from left to right, how does the
metallic character of elements change?
•a) It increases.
•b) It decreases. ✅
•c) It remains the same.
•d) It fluctuates.
metallic character of elements change?
•a) It increases.
•b) It decreases. ✅
•c) It remains the same.
•d) It fluctuates.
•Which of the following is most
characteristic of metalloids?
•a) They are good conductors of electricity.
•b) They have properties that are intermediate
between metals and nonmetals. ✅
•c) They readily gain electrons.
•d) They are highly reactive metals
characteristic of metalloids?
•a) They are good conductors of electricity.
•b) They have properties that are intermediate
between metals and nonmetals. ✅
•c) They readily gain electrons.
•d) They are highly reactive metals
•Which of the following elements is a
metalloid?
•a) Aluminum (Al)
•b) Silicon (Si) ✅
•c) Magnesium (Mg)
•d) Helium (He)
metalloid?
•a) Aluminum (Al)
•b) Silicon (Si) ✅
•c) Magnesium (Mg)
•d) Helium (He)
•Which of the following elements is most
likely to exhibit nonmetallic character?
•a) Iron (Fe)
•b) Sulfur (S) ✅
•c) Zinc (Zn)
•d) Calcium (Ca)
likely to exhibit nonmetallic character?
•a) Iron (Fe)
•b) Sulfur (S) ✅
•c) Zinc (Zn)
•d) Calcium (Ca)
•Which of the following properties
increases as you move across a period
from left to right?
•a) Metallic character.
•b) Electronegativity. ✅
•c) Atomic radius.
•d) Ionization energy.
increases as you move across a period
from left to right?
•a) Metallic character.
•b) Electronegativity. ✅
•c) Atomic radius.
•d) Ionization energy.
•Which of the following elements is most
likely to form an anion with a charge of -
1?
•a) Calcium (Ca)
•b) Oxygen (O) ✅
•c) Sodium (Na)
•d) Magnesium (Mg)
likely to form an anion with a charge of -
1?
•a) Calcium (Ca)
•b) Oxygen (O) ✅
•c) Sodium (Na)
•d) Magnesium (Mg)
•Which of the following elements would
likely have a high ionization energy and
high electronegativity?
•a) Lithium (Li)
•b) Fluorine (F) ✅
•c) Sodium (Na)
•d) Potassium (K)
likely have a high ionization energy and
high electronegativity?
•a) Lithium (Li)
•b) Fluorine (F) ✅
•c) Sodium (Na)
•d) Potassium (K)
•Which trend is observed as you move
down a group of the periodic table in
terms of metallic character?
•a) Metallic character increases. ✅
•b) Metallic character decreases.
•c) Metallic character remains the same.
•d) Metallic character fluctuates.
down a group of the periodic table in
terms of metallic character?
•a) Metallic character increases. ✅
•b) Metallic character decreases.
•c) Metallic character remains the same.
•d) Metallic character fluctuates.
•Which element in Period 2 is most likely
to behave as a nonmetal in reactions?
•a) Boron (B)
•b) Carbon (C)
•c) Nitrogen (N)
•d) Fluorine (F) ✅
to behave as a nonmetal in reactions?
•a) Boron (B)
•b) Carbon (C)
•c) Nitrogen (N)
•d) Fluorine (F) ✅
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