The Atomic structure,Ionisation and formig of simple Ionic bonds.

PPT covering Atomic structure and Ionisation. Covers forming ions,electronic configuration and formation of simple ionic bonds

1. Atoms and Bonding What are they and what do they do?

2. KEYWORDS Atom Element Matter Compound Bonding Molecule Atomic number Neutron Atomic mass Nucleus Electron Proton Neutron

3. Everything is made up of matter. An atom is the building block of all matter. Each element is made up of only one type of atom.

4. Matter Anything that has mass and takes up space (volume) Examples: A desk has mass and takes up space Water has mass and takes up space Air has mass and takes up space Can you think of anything that would not be considered matter?

5. Atoms Matter is made up of atoms . An atom is the smallest possible unit into which matter can be divided, while still maintaining its properties. An atom is Made up of: protons neutrons Electrons When 2 or more atoms combine, a molecule is produced. + + + - - - - +

6. An element is a substance that is made up of only one type of atom. So far there are 118 different elements that have been discovered. The periodic table contains a list of all known elements. ELEMENT

7. Protons (+) Positively charged particles(+) Found in the nucleus of the atom Equal to the atomic number of the atom Contribute to the atomic mass Its equal to number of electroins to the number of electrons + + + + + + + + - - - - - - - - +

8. Neutrons Neutral particles; have no electric charge(Neutral) Found in the the nucleus of the atom Contribute to the atomic mass + + + + + + + - - - - - - - - +

9. Electrons (-) Negatively charged particles(-) Found outside the nucleus of the atom, in the shells . Equal to the number of protons. Involved in the formation of chemical bonds - + + + + + + + - - - - - - - - +

10. The Atom’s “Center” Protons and neutrons are grouped together to form the “center” or nucleus of an atom. - + + + Notice that the electrons are not apart of the nucleus - -

11. Atomic Number The number of protons in the nucleus of an atom + + + - - - What would be the atomic number of this atom?

12. Mass Number The total number of protons and neutrons in an atom’s nucleus Expressed in A tomic M ass U nits (amu) Each proton or neutron has a mass of 1 amu + + + - - - What would be the mass number of this atom? +  3  4 3 protons + 4 neutrons = a mass number of 7 amu

13. Where do we find the electrons in an atom? Th electrons are negatively charged. They are located outside the nucleus Electrons are arranged in shells. 1st Shell: Fills this first 2 nd Shell: Fill this next 3 rd Shell: And so on

14. Differences between the parts Proton Charge: Positive +1 Mass: Heavier Location: Nucleus Role in the atom: Helps identify the element Neutron Charge: 0 Mass: About the same as proton which is heavy Location: Nucleus Role in the atom: Help hold everything together Electron Charge: Negative -1 Mass:Just about nothing Location: Outside of the Nucleus Role in the atom: Chemical reactivity of the atom

15. How to find: Number of Protons Same as Atomic Number Mass Number Protons + Neutrons Number of Neutrons Mass Number - Atomic Number Number of Electrons Same as number of Protrons

16. Chemical Symbols Chemical symbols are used to represent elements on the periodic table. Each element has its own symbol that is different from all other chemical symbols.

17. Particle Relative Mass Relative Charge Proton 1 +1 Neutron 1 Electron -1 He 2 4 MASS NUMBER number of protons + number of neutrons SYMBOL PROTON NUMBER /(Atomic number) number of protons (same as electrons)

18.   6 C 12 11 Na 23 Atomic number = 6 Atomic mass = 12.01 (round to 12) Number of neutrons = 6 Number of Electrons = 6 Atomic number = 11 Atomic mass = 23 Number of neutrons = 12 Number of electrons = 11

19. Calculating the number of protons, neutrons and electrons. How many protons? 3 – Number of protons = atomic number How many electrons? 3 – Number of electrons = number of protons (atomic number How many neutrons? 4 - The nucleus is made up of P+N (mass no. = 7). Mass number – atomic number = number of neutrons Li 7 3

20. Practice Questions Prove the learning Number of protons in Aluminium: Number of neutrons in Carbon: Number of electrons in Carbon: Number of electrons in Oxygen: Number of protons in Oxygen: Number of neutrons in Sulfur : Number of electrons in Lithium: Number of electrons in Chlorine: Number of protons and neutrons in Chlorine: Number of protons and electrons in Lithium: Write 3 more questions of your own. Get a partner to answer them – give them feedback .

21. Hydrogen (H) Atom Notice the one electron in the first shell + - What is it lacking? + - = 1 = 0 = 1 How many more electrons can fit in the 1 st Shell

22. Oxygen (O) Atom Notice the two electrons (e ) in the first Shell and the six in the second + + + + + + + - - - - - - - - + + - = 8 = 8 = 8 How many more electrons can fit in the 2 nd shell?

23. Sodium (Na) Atom Notice the two electrons in the 1st Shell, eight in the second, and one in the third + + + + + + + - - - - - - - - + - - - + - = 11 = 12 = 11 How many more electrons can fit in the 3 rd shell?

24. Study Tip: Protons and Neutrons Number of protons = Atomic number Number of protons + neutrons = Mass number Number of neutrons = mass number – atomic number (protons)

25. SUMMARY The Atomic Number of an atom = number of protons in the nucleus. The Mass number of an atom = number of Protons + Neutrons in the nucleus. The number of Protons = Number of Electrons. Electrons moves around the nucleus in shells . Each shell can only carry a set number of electrons.

26. Rules Maximum number of electrons that can be accommodated in a shell . For 1 st  shell, n = Maximum number of electrons is 2 For 2 nd  shell n = Maximum number of electrons is 8 For 3 rd   shell n = Maximum number of electron is 8

27. Where do we find the electrons in an atom? Th electrons are negatively charged. They Electrons will occupy the lowest shell first (the shells nearest the nucleus) unless these shells are already full. 1st Shell: Fills this first 2 nd Shell: Fill this next 3 rd Shell: And so on

28. Drawing Electronic Structures 1 st Shell Capacity = 2 2 nd Shell Capacity = 8 3 rd Shell Capacity = 8 4 th Shell Capacity = 2 The electrons in an atom occupy energy levels. These are also called shells . The lowest energy level (innermost shell) fills with electrons first.

29. Drawing electronic structures Each shell has a maximum number of electrons that it can hold. 1 st Shell: 2 nd Shell: 3 rd Shell: 4 th Shell: H x x He 2 x x x x x x x x Ne x x x x x x x x Ar 8 8 x x Ca 2 You need to be able to draw the electronic structure for the first 20 elements!

30. How do we draw the electronic structure for….. Oxygen How do we write the electronic structure? O 16 8 2:6 You need to ask yourself… How many electrons are there in total? What period is it in? (how many shells does it have?) What group is it in? (how many electrons are there in the outer shell?)

31. ELECTRONIC CONFIGURATION With electronic configuration elements are represented numerically by the number of electrons in their shells and number of shells. For example; N Nitrogen 14 2 in 1 st shell 5 in 2 nd shell configuration = 2 , 5 2 + 5 = 7 7

32. ELECTRONIC CONFIGURATION Write the electronic configuration for the following elements; Ca O Cl Si Na 20 40 11 23 8 17 16 35 14 28 B 11 5 a) b) c) d) e) f) 2,8,8,2 2,8,1 ??? ??? ??? 2,6 O

33. DOT & CROSS DIAGRAMS With Dot & Cross diagrams elements and compounds are represented by Dots or Crosses to show electrons, and circles to show the shells. For example; N 7 14

34. DOT & CROSS DIAGRAMS Draw the Dot & Cross diagrams for the following elements; O Cl 8 16 35

35. Octet Rule The outermost shell of an atom cannot accommodate more than 8 electrons, even if it has a capacity to accommodate more electrons. This is a very important rule and is also called the Octet rule. The presence of 8 electrons in the outermost shell makes the atom very stable.

36. Work out the electronic structure of the following, using the 2,8,8….. method. Lithium Chlorine Argon Sulphur Boron Aluminium

37. How do we draw the electronic structure for….. Carbon How do we write the electronic structure? 2,4 C 12 6

38. How do we draw the electronic structure for….. Magnesium How do we write the electronic structure? 2,8,2 Mg 24 12

39. TASK Prove the learning Draw electronic structures for the following elements Sodium (Na) Calcium ( Ca ) Nitrogen (N) Chlorine ( Cl ) For each one you need to ask yourself… How many electrons are there in total? What period is it in? (how many shells does it have?) What group is it in? (how many electrons are there in the outer shell?)

40. How can reactive atoms become stable?

41. What is an Ion? An ion is an atom or group of atoms that has an electrical charge, either positive and negative. Atoms with incomplete outer electron shells are unstable. (They need to have 8 electrons in their outer shell or 2 electrons if they have 1 shell. By either gaining or losing electrons, atoms can obtain full outer electron shells and become stable.

42. An atom that loses electrons has more protons than electrons and so has a positive overall charge. This is called a positive ion . An atom that gains electrons has more electrons than protons and so has a negative overall charge. This is called a negative ion .

43. Ions An ion is formed when an atom gains or loses electrons and becomes charged: If we “take away” the electron we’re left with just a positive charge: This is called an ion (in this case, a positive hydrogen ion) + - + The electron is negatively charged The proton is positively charged +

44. Simple Ions Cations Sodium – Na + Magnesium – Mg 2+ Iron – Fe 3+ Copper – Cu 2+ Anions Chloride – Cl - Sulphate – SO 4 2- Carbonate – CO 3 2- Oxide – O 2-

45. Remember - Atoms like to have FULL electron shells!!

46. How is a sodium ion formed? 2.8.1 (partially full outer shell) 11 protons = +11 11 electrons = -11 Total charge = 0 Sodium atom: 11 protons = +11 10 electrons = -10 Total charge = +1 Sodium ion: loses 1 electron + [2.8] (full outer shell) Na Na

47. How is a magnesium ion formed? 2.8.2 (partially full outer shell) 12 protons = +12 12 electrons = -12 Total charge = 0 Magnesium atom: 12 protons = +12 10 electrons = -10 Total charge = +2 Magnesium ion: [2.8] 2+ (full outer shell) 2+ Mg Mg loses 2 electrons

48. How is a fluoride ion formed? 2.7 (partially full outer shell) 9 protons = +9 9 electrons = -9 Total charge = 0 Fluorine atom: 9 protons = +9 10 electrons = -10 Total charge = -1 Fluoride ion: [2.8] - (full outer shell) - F F gains 1 electron

49. [2.8.8] 2- (full outer shell) 2.8.6 (partially full outer shell) How is a sulfide ion formed? 16 protons = +16 16 electrons = -16 Total charge = 0 Sulfur atom: 16 protons = +16 18 electrons = -18 Total charge = -2 Sulfide ion: 2- S S gains 2 electrons

50. Losing electrons to form positive ions… x x xx xx xx x 2,8,1 Sodium Na Na + 2,8 A sodium atom has 11 protons and so 11 electrons. It needs to lose one electron to get a full outer shell. The sodium ion still has 11 protons in its nucleus but now has only 10 electrons. 11 positive protons – 10 negative electrons = +1 charge Electronic configuration xx

51. GROUP 1:THE ALKALI METALS

52. Losing electrons to form positive ions… A calcium atom has 20 protons and so 20 electrons. It needs to lose two electrons to get a full outer shell. The calcium ion still has 20 protons in its nucleus but now has only 18 electrons. 20 positive protons – 18 negative electrons = +2 charge 2,8,8,2 Calcium Ca 2+ 2,8,8 x x xx xx xx Ca xx x x Electronic configuration xx xx xx xx

53. Gaining electrons to form negative ions… A chlorine atom has 17 protons and so 17 electrons. It needs to gain one electron to get a full outer shell. The chloride ion still has 17 protons in its nucleus but now has 18 electrons. 17 positive protons – 18 negative electrons = -1 charge x x xx xx xx x 2,8,7 Chlorine Cl Cl - 2,8,8 x Electronic configuration xx xx xx xx

54. HALOGENS GROUP 7

55. Gaining electrons to form negative ions… A oxygen atom has 8 protons and so 8 electrons. It needs to gain two electrons to get a full outer shell. The oxide ion still has 8 protons in its nucleus but now has 10 electrons. 8 positive protons – 10 negative electrons = -2 charge x x 2,6 Oxygen O O 2- 2,8 Electronic configuration xx xx xx xx

56. NOBLE GASES

57. L3 The Periodic Table 2 What ion is formed, and draw and write out the electron configuration, when these become ions… Sodium  Potassium Beryllium Chlorine Sulfur Aluminium Calcium What happens with argon??? You try some Na + {2,8}, cation

58. What is Ionic Bonding? These compounds are usually formed by a reaction between a metal and a non-metal . The metal and non-metal atoms have incomplete outer electron shells and so are unstable . The positive and negative ions are strongly attracted to each other. This electrostatic attraction is called ionic bonding .

59. Ionic Compounds An ionic compound is a compound that is formed by ionic bonding. Ionic bonding occurs through a process called electron transfer , where one atom gives electrons to another. In electron transfer, an atom of one element loses one or more electrons, and an atom of another element gains those electrons. Both of the atoms involved in electron transfer become ions.

60. A match made in heaven… Metal atoms want to lose electrons… Non-metals atom want to gain electrons… For example, A sodium atom is desperate to lose an electron… A chlorine atom is desperate to gain an electron… Na + Cl -

61. Dot and Cross Diagrams NaCl – Sodium Chloride - Cl Na +

62. What is the ratio of ions? Sodium chloride (NaCl) and magnesium oxide (MgO) are simple ionic compounds. Both compounds have a 1:1 ratio of metal ions to non-metal ions Na Cl Na + Cl - 1 electron Mg Mg 2+ O O 2- 2 electrons In each compound, the metal needs to lose the same number of electrons that the non-metal needs to gain .

63. What is the ratio of ions in sodium oxide? Sodium (2.8.1) needs to lose 1 electron to form a sodium ion but oxygen (2.6) must gain 2 electrons to form an oxide ion . Na Na O O 2- Na + Na + 1 electron from each Na atom Two sodium atoms are required for each oxygen atom and so the ratio of sodium ions to oxide ions is 2:1. From this ratio, the formula of sodium oxide is Na 2 O.

64. What is the ratio of ions in magnesium chloride? Magnesium (2.8.2) needs to lose 2 electrons to form a magnesium ion but chlorine (2.8.7) needs to gain 1 electron to form an chloride ion. Mg Cl Mg 2+ Cl Cl - Cl - 1 electron for each Cl atom Two chlorine atoms are required for each magnesium atom and so the ratio of magnesium ions to chloride ions is 1:2. From this ratio, the formula of magnesium chloride is MgCl 2 .

65. How to show the transfer of electrons. There two types of ions formed n amely : Metals form Cations - Positive charged ions Non –metals form Anions - Negatively charged ions

66. What are ions? Here is a sodium atom and a sodium ion Here is a chlorine atom and a chloride ion

67. Ions are charged particles When metal atoms and non-metal atoms bond together they form charged particles called ions. They have a different number of electrons to protons so they have either a positive or negative charge. Metals always form positive ions. Complete electron arrangements in atoms and ions worksheet from hard copy C2 folder

68. Starter: Questions: Draw the electronic structure of Magnesium How many neutrons are there in Aluminium? How many electrons are there in sodium? What group is Boron in? What period is potassium in? How many electron shells in Fluorine? How many electrons in the outer shell of Chlorine? Describe the properties/reactivity of Barium Describe the properties of cobalt Draw the electronic structure of a calcium ion

69. Noble gases K+U LOs Describe the trends in group 0 Explain the trends in group 0 PLTs Self Managers Effective Participators 22/10/2025

70. Noble gases Can you describe their properties? How could you test them? What do they look like? Smell like?

71. Noble gases All noble gases are monatomic, colourless, odourless and unreactive. This makes them difficult to isolate and identify They’re useful because they’re unreactive Earth’s atmosphere contains tiny amounts of Noble Gases Group 0 in Periodic table – full outer shells

72. Uses of noble gases Although noble gases are unreactive, they are still very useful elements. Many uses of noble gases depend on their ability to prevent other, undesirable, reactions taking place.

73. Uses of helium It is used for inflating balloons and airships. It is safer than it’s only alternative, hydrogen, because its low reactivity means that it does not catch fire! It is a component of breathing gas (with oxygen) for deep-sea divers, because it is unreactive, insoluble and prevents divers getting ‘the bends’.

74. Uses of neon Neon is used in neon lights, because it gives a bright light when an electric current is passed through it.

75. Uses of argon Use in normal light bulbs, because it is unreactive and prevents the tungsten filament from burning. When you pass a current through the metal filament, the metal becomes white hot. However, because argon is inert (unreactive), no chemical reaction takes place. This stops the filament from burning away and makes light bulbs last longer.

76. Noble gas Use Helium Neon Argon Krypton Xenon Radon Very low density – filling balloons Bright light when electric current passed through it - advertising Very unreactive – environment in light bulbs Lighthouse bulbs (not for killing Superman) Electron tubes and lasers Very radioactive - radiotherapy

77. Noble gases Tasks: D: List properties and uses of noble gases C: Describe why noble gases are useful – give examples B: C grade +… describe the trends in group 0 A/A*: C and B grade +… explain the trends in group 0 https://www.youtube.com/watch?v=jdzBRmLsUM8 https://www.youtube.com/watch?v=Lid8BsbqTDQ

78. Group 1 metals K+U LOs Describe what a ‘group’ is and explain why elements are arranged in groups. PLTs Self Managers Effective Participators 05/09/2012 Success Criteria Define the terms group and period.

79. Groups and periods Horizontal rows are called PERIODS Vertical columns are called GROUPS Groups – gro ’ UP ! Periods – PER – P eriods E quals R ows.

80. Watch and be ready to take notes ! Watch the demo If you have a question or something to say, share it. Let the person talk! (Don’t interrupt.) Listen. If it has to be said then say it to the class ! Why are elements grouped together? What do the atoms in a group have in common? Why might elements in the same group react in the same way as each other? do the same things as each other? Demo/whiteboards

81. Describing the trend in reactivity of group 1 elements All the elements in group 1…… As you go down group 1, the elements get…. I know this because…. Prove the learning

82. 5 Minute Task Explain what these atoms have in common Lithium Sodium Potassium Elements with the same chemical properties are grouped together. Elements in the same group all react in the same way because… 2,1 2,8,1 2,8,8,1

83. PREDICT the reaction of caesium and water http://www.youtube.com/watch?v=QSZ-3wScePM

84. Group 7 – the halogens The elements in group 7 of the periodic table, on the right, are called the halogens . fluorine chlorine bromine iodine astatine I Br Cl F At

85. How do halogen molecules exist? All halogen atoms require one more electron to obtain a full outer shell and become stable. Each atom can achieve this by sharing one electron with another atom to form a single covalent bond . This means that all halogens exist as diatomic molecules: F 2 , Cl 2 , Br 2 and I 2 . +  F F F F

86. Halogens – what do they look like? Chlorine Bromine Iodine

87. Halogen vapours Bromine and iodine are not gaseous, but have low boiling points. This means that they produce vapour at relatively low temperature. They are volatile . Bromine produces some red-brown vapour, seen here above the liquid bromine in the jar. When iodine is heated gently, it changes directly from a solid to a gas without first becoming a liquid. This is called sublimation .

88. State and colour at room temperature   What is the state and colour of each of the following Group VII elements at room temperature?   Chlorine _____________ Bromine _____________ Iodine _____________   Melting points and boiling points   What happens to the melting + boiling points of the Halogens as you go down Group VII? __________________________________________________________________________  

89. Halogens continued… Answer these questions in your book What colour is chlorine, bromine and iodine Halogens go around in pairs – what word describes molecules made up of 2 atoms? Draw a dot and cross diagram showing the bonding in a molecule of Fluorine (F 2 )

90. Halogen displacement reactions Bearing in mind that reactivity decreases down group 7. Draw this table and predict which halogens will displace other halogens from a salt

91. Displacement reactions: summary halogen chlorine bromine iodine salt (aq) potassium chloride potassium iodide potassium bromide Yes no reaction no reaction no reaction Yes Yes

92. Transition metals Transition metals https://www.youtube.com/watch?v=56DyU-46OKw

93. Transition metals… True or false? Usually have low melting points Usually have high melting points Are all magnetic Are all solids at room temperature (apart from mercury) Are usually strong Are found in groups 1 and 2 of the periodic table Are usually dense (heavy) Are found in the middle of the periodic table Examples are potassium, aluminium and sodium Examples are iron, silver and titanium Are usually good conductors of heat and electricity Are usually good insulators of heat and electricity Have lots of uses (including being used as catalysts to help speed up reactions) Are usually malleable (can be bent into shapes) Are usually ductile (can be stretched into wires)

94. Transition metals… True or false? Usually have low melting points Usually have high melting points Are all magnetic Are all solids at room temperature (apart from mercury) Are usually strong Are found in groups 1 and 2 of the periodic table Are usually dense (heavy) Are found in the middle of the periodic table Examples are potassium, aluminium and sodium Examples are iron, silver and titanium Are usually good conductors of heat and electricity Are usually good insulators of heat and electricity Have lots of uses (including being used as catalysts to help speed up reactions) Are usually malleable (can be bent into shapes) Are usually ductile (can be stretched into wires)

95. These elements can form different ions. Compounds of these ions are different colours.