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AS Chemistry The Periodic Table.

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1 AS Chemistry The Periodic Table

2 THE PERIODIC TABLE = the elements arranged in rows (PERIODS)
in order of increasing atomic number (Z) such that chemically similar elements occur in the same vertical columns (GROUPS).

3 Group 1 Group 2 Group 3 Group 4 Group 5 Group 6 Group 7 Group 0 Period 1 Period 2 Period 3 Period 4 Period 5 Period 6 Period 7

4 s-block p-block d-block

5 GROUP = elements within the same vertical column
Chemical and physical properties are similar within a group Group number = number of electrons in highest occupied energy level e.g. Group I eg Na[2,8,1] = the alkali metals Group VII eg F[2,7] = the halogens

6 ? AS Chemistry Trends in Physical Properties of Group 2 Metals Mg Ca
Sr Ba Trends in Physical Properties of Group 2 Metals

7 INCREASES as EXTRA e- SHELLS ADDED which are INCREASINGLY SHIELDED from the nucleus.

8 INCREASES as EXTRA e- SHELLS ADDED which are INCREASINGLY SHIELDED from the nucleus.

9 INCREASES as EXTRA e- SHELLS ADDED which are INCREASINGLY SHIELDED from the nucleus.

10 INCREASES as EXTRA e- SHELLS ADDED which are INCREASINGLY SHIELDED from the nucleus.

11 M (g)  M+(g) + e- DECREASES because the outer e- is more distant and more shielded from attracting nuclear protons, even though more p+ are present. This causes a WEAKER attractive force and consequently, a lowering of ionisation energy

12 M (g)  M+(g) + e- DECREASES because the outer e- is more distant and more shielded from attracting nuclear protons, even though more p+ are present. This causes a WEAKER attractive force and consequently, a lowering of ionisation energy

13 M (g)  M+(g) + e- DECREASES because the outer e- is more distant and more shielded from attracting nuclear protons, even though more p+ are present. This causes a WEAKER attractive force and consequently, a lowering of ionisation energy

14 Mg unusual because atoms DO NOT pack together as well as others
DECREASE A s metallic bonding gets WEAKER because radius and mass of the 2+ ions INCREASE  attractions between 2+ cations and the 2 delocalised electrons per atom become WEAKER.

15 Mg unusual because atoms DO NOT pack together as well as others
DECREASE A s metallic bonding gets WEAKER because radius and mass of the 2+ ions INCREASE  attractions between 2+ cations and the 2 delocalised electrons per atom become WEAKER.

16 Mg unusual because atoms DO NOT pack together as well as others
DECREASE A s metallic bonding gets WEAKER because radius and sheilding of the 2+ ions INCREASE  attractions between 2+ cations and the 2 delocalised electrons per atom become WEAKER.

17 PERIOD = elements within the same horizontal row
Chemical and physical properties change from extremes across any period. e.g. Period 3 Sodium = a reactive metallic solid Argon = an unreactive, non- metallic gas Period number = number of shells eg Si (Z=14)  2,8,4  Period 3 and Group 4

18 Atomic radius DECREASES across period 3.
Outer e- in same energy level (distance & shielding similar) but attracted more strongly as no. of nuclear protons increases

19 MELTING POINT

20 MELTING POINT Boiling and melting points are a measure of the energy required to separate the particles in a substance. Bond type is significant. Kelvin Periods A general increase then a decrease SODIUM MAGNESIUM 3000 2500 2000 1500 1000 500 Na Mg Al Si P S Cl Ar

21 MELTING POINT Boiling and melting points are a measure of the energy required to separate the particles in a substance. Bond type is significant. Kelvin Periods A general increase then a decrease Metals Na-Al Melting point increases due to the increasing strength of metallic bonding caused by ... the larger number of electrons contributing to the “cloud” larger charge and smaller size of ions gives rise to a larger charge density. SODIUM MAGNESIUM 3000 2500 2000 1500 1000 500 Na Mg Al Si P S Cl Ar The electron cloud in magnesium is denser than in sodium so more energy is required to separate the ‘ions’

22 MELTING POINT Boiling and melting points are a measure of the energy required to separate the particles in a substance. Bond type is significant. Kelvin Periods A general increase then a decrease Metals Na-Al Melting point increases due to the increasing strength of metallic bonding caused by ... the larger number of electrons contributing to the “cloud” larger charge and smaller size of ions gives rise to a larger charge density. SODIUM MAGNESIUM 3000 2500 2000 1500 1000 500 Na Mg Al Si P S Cl Ar The electron cloud in magnesium is denser than in sodium so more energy is required to separate the ‘ions’

23 MELTING POINT Boiling and melting points are a measure of the energy required to separate the particles in a substance. Bond type is significant. Non-metals Si-Ar SILICON Large increase in melting point as it has a giant molecular structure like diamond A lot of energy is required to break the many covalent bonds holding the atoms together. Kelvin 3000 2500 2000 1500 1000 500 Na Mg Al Si P S Cl Ar

24 MELTING POINT Boiling and melting points are a measure of the energy required to separate the particles in a substance. Bond type is significant. P, S, Cl, Ar Very much lower melting points as they are simple covalent molecules Melting point depends on the weak intermolecular van der Waals’ forces. The larger the molecule the greater the van der Waals’ forces P S Cl2 relative mass melting point °C 119°C °C Kelvin 3000 2500 2000 1500 1000 500 Na Mg Al Si P S Cl Ar

25 MELTING POINT Boiling and melting points are a measure of the energy required to separate the particles in a substance. Bond type is significant. PHOSPHORUS can exist is several allotropic forms. In the most common, red phosphorus, each molecule exists in a tetrahedral structure. The atoms are joined by covalent bonds within the molecule formula P4 relative mass 124 melting point 44°C Melting point drops dramatically as intermolecular attractions are now due to weak van der Waals’ forces. Kelvin 3000 2500 2000 1500 1000 500 Na Mg Al Si P S Cl Ar

26 MELTING POINT Boiling and melting points are a measure of the energy required to separate the particles in a substance. Bond type is significant. SULPHUR can exist is several allotropic forms. Sulphur usually exists in a puckered eight membered ring structure. The atoms are joined by covalent bonds within the molecule formula S8 relative mass 256 melting point °C Melting point rises slightly as the molecule is bigger so has slightly stronger van der Waals’ forces. Kelvin 3000 2500 2000 1500 1000 500 Na Mg Al Si P S Cl Ar

27 MELTING POINT Boiling and melting points are a measure of the energy required to separate the particles in a substance. Bond type is significant. CHLORINE Exists as a linear diatomic molecule. The atoms are joined by covalent bonds within the molecule formula Cl2 relative mass 71 melting point °C Melting point falls slightly as the molecule is smaller so has slightly lower van der Waals’ forces. Kelvin 3000 2500 2000 1500 1000 500 Na Mg Al Si P S Cl Ar

28 MELTING POINT Boiling and melting points are a measure of the energy required to separate the particles in a substance. Bond type is significant. ARGON Exists as a monatomic species. formula Ar relative mass 40 melting point °C Melting point falls. Kelvin 3000 2500 2000 1500 1000 500 Na Mg Al Si P S Cl Ar

29 MELTING POINT TREND - NON METALS
P S Cl Ar relative mass melting point / K

30 BOILING POINT Boiling and melting points are a measure of the energy required to separate the particles in a substance. Bond type is significant. Boiling points tend to be a better measure and show better trends because solids can be affected by the crystal structure as well as the type of bonding. As is expected, the boiling points are higher than the melting points. Kelvin 3000 2500 2000 1500 1000 500 Na Mg Al Si P S Cl Ar

31 BOILING POINT Boiling and melting points are a measure of the energy required to separate the particles in a substance. Bond type is significant. Boiling points tend to be a better measure and show better trends because solids can be affected by the crystal structure as well as the type of bonding. As is expected, the boiling points are higher than the melting points. Kelvin 3000 2500 2000 1500 1000 500 Na Mg Al Si P S Cl Ar

32 BOILING POINT Boiling and melting points are a measure of the energy required to separate the particles in a substance. Bond type is significant. Note the trend from Al – Si varies slightly when we consider the mpt trend and the bpt trend. The mpt increases from Al – Si but the bpt decreases. The is because when Silicon melts many of its covalent bonds are broken so to vaporize molten silicon does not require as much energy as to vaporize molten Aluminium Kelvin 3000 2500 2000 1500 1000 500 Na Mg Al Si P S Cl Ar

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40 Giant Metallic Giant Covalent Simple Covalant

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