Introduction chemistry section powerpoint presentation

Atom vs Molecules

1. Atoms vs. Molecules
Matter is composed of tiny particles called atoms.
Atom: smallest part of an element that is still that
element.
Molecule: Two or more atoms joined and acting as a
unit.
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2. Oxygen and Hydrogen
Molecules
•Use subscripts when more than one atom is in the
molecule.
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3. A Chemical Reaction
One substance changes to another by reorganizing the
way the atoms are attached to each other.
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4. Atomic Theory
Atoms are building blocks of elements
Similar atoms in each element
Different from atoms of other elements
Two or more different atoms bond in simple
ratios to form compounds
4

5. Subatomic Particles
ParticleSymbol Charge Relative
Mass
Electrone
-
1- 0
Proton p
+
+ 1
Neutronn 0 1
5

6. Location of Subatomic Particles
10
-13
cm
electrons
protons
neutrons
10
-8
cm
6
nucleus

7. Atomic NumberThis refers to how
many protons an
atom of that element
has.
No two elements,
have the same
number of protons.
Bohr Model of Hydrogen Atom
Wave Model

8. Atomic Number on the Periodic Table
11
Na
8
Atomic Number
Symbol

9. All atoms of an element have the
same number of protons
11
Na
9
11 protons
Sodium

10. Learning Check
State the number of protons for atoms of each
of the following:
A. Nitrogen
B. Sulfur
C. Barium
10

11. Solution
State the number of protons for atoms of each
of the following:
A. Nitrogen
7 protons
B. Sulfur
16 protons
C. Barium
56 protons
11

12. Mass Number
Counts the number
of
protons and neutrons
in an atom
12

13. Atomic Symbols
Show the mass number and atomic number
Give the symbol of the element
mass number
23
Na sodium-23
atomic number
11
13

14. Number of Electrons
An atom is neutral
The net charge is zero
Number of protons = Number of electrons
Atomic number = Number of electrons
14

15. Subatomic Particles in Some Atoms
16 31 65
O P Zn
8 15 30
8 p
+
15 p
+
30 p
+
8 n 16 n 35 n
8 e
-
15e
-
30 e
-
15

16. Isotopes
Atoms with the same number of protons but
different numbers of neutrons.
Show almost identical chemical properties;
chemistry of atom is due to its electrons.
In nature most elements contain mixtures of
isotopes.
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17. Atomic Mass and
Isotopes
While most atoms have the
same number of protons
and neutrons, some don’t.
Some atoms have more or
less neutrons than protons.
These are called isotopes.
An atomic mass number
with a decimal is the total
of the number of protons
plus the averagenumber of
neutrons.

18. Two Isotopes of Sodium
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19. Isotopes
Atoms with the same number of protons, but
different numbers of neutrons.
Atoms of the same element (same atomic
number) with different mass numbers
Isotopes of chlorine
35
Cl
37
Cl
17 17
chlorine -35 chlorine -37
19

20. Learning Check
Naturally occurring carbon consists of three
isotopes,
12
C,
13
C, and
14
C. State the number of
protons, neutrons, and electrons in each of these
carbon atoms.
12
C
13
C
14
C
6 6 6
#p _______ _______ _______
#n _______ _______ _______
#e _______ _______ _______
20

21. Solution
12
C
13
C
14
C
6 6 6
#p 6 6 6
#n 6 7 8
#e 6 6 6
21

22. Learning Check
An atom of zinc has a mass number of 65.
A.What is the number of protons in the zinc
atom?
B.What is the number of neutrons in the zinc
atom
C. What is the mass number of a zinc isotope
with 37 neutrons?
22

23. Solution
An atom of zinc has a mass number of 65.
A.Number of protons in the zinc atom
30
B.Number of neutrons in the zinc atom
35
C. What is the mass number of a zinc isotope
with 37 neutrons?
67
23

24. Learning Check
Write the atomic symbols for atoms with
the following:
A. 8 p
+
, 8 n, 8 e
-
___________
B.17p
+
, 20n, 17e
-
___________
C. 47p
+
, 60 n, 47 e
-
___________
24

25. Solution
16
O
A. 8 p
+
, 8 n, 8 e
- 8
B.17p
+
, 20n, 17e
- 37
Cl
17
C. 47p
+
, 60 n, 47 e
-107
Ag
47
25