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periodicity, structure and bonding

Total questions: 45

Worksheet time: 30mins

Name
Class
Date
1.

Lithium (Li)

a)

Metallic

b)

Colvalent molecular

c)

Colvalent network

d)

Monatomic

2.

Beryllium (Be)

a)

Metallic

b)

Colvalent molecular

c)

Colvalent network

d)

Monatomic

3.

Sodium (Na)

a)

Metallic

b)

Colvalent molecular

c)

Colvalent network

d)

Monatomic

4.

Magnesium (Mg)

a)

Metallic

b)

Colvalent molecular

c)

Colvalent network

d)

Monatomic

5.

Aluminium (Al)

a)

Metallic

b)

Colvalent molecular

c)

Colvalent network

d)

Monatomic

6.

Potassium (K)

a)

Metallic

b)

Colvalent molecular

c)

Colvalent network

d)

Monatomic

7.

Calcium (Ca)

a)

Metallic

b)

Colvalent molecular

c)

Colvalent network

d)

Monatomic

8.

Hydrogen(H2)

a)

Metallic

b)

Colvalent molecular

c)

Colvalent network

d)

Monatomic

9.

Nitrogen(N2)

a)

Metallic

b)

Colvalent molecular

c)

Colvalent network

d)

Monatomic

10.

Oxygen(O2)

a)

Metallic

b)

Colvalent molecular

c)

Colvalent network

d)

Monatomic

11.

Fluorine (F2)

a)

Metallic

b)

Colvalent molecular

c)

Colvalent network

d)

Monatomic

12.

Phosphorus (P4)

a)

Metallic

b)

Colvalent molecular

c)

Colvalent network

d)

Monatomic

13.

sulfur(S8)

a)

Metallic

b)

Colvalent molecular

c)

Colvalent network

d)

Monatomic

14.

Chlorine (Cl2)

a)

Metallic

b)

Colvalent molecular

c)

Colvalent network

d)

Monatomic

15.

Fullerenes

a)

Metallic

b)

Colvalent molecular

c)

Colvalent network

d)

Monatomic

16.

Boron(B)

a)

Metallic

b)

Colvalent molecular

c)

Colvalent network

d)

Monatomic

17.

Carbon (C, diamond, graphite)

a)

Metallic

b)

Colvalent molecular

c)

Colvalent network

d)

Monatomic

18.

Silicone (Si)

a)

Metallic

b)

Colvalent molecular

c)

Colvalent network

d)

Monatomic

19.

Nobel gases

a)

Metallic

b)

Colvalent molecular

c)

Colvalent network

d)

Monatomic

20.

Name the element from the third period that exists as a covalent network.

(a)  

21.

Explain why the covalent radius of sulfur is smaller than that of phosphorus.

a)

Increased nuclear attraction for electrons

b)

increased nuclear charge

c)

sulfur has more protons in nucleus

d)

increased attraction of electrons for nucleus

22.

Explain fully, in terms of the structures of sulfur and phosphorus molecules and the intermolecular forces between molecules of each element, why the melting point of sulfur is much higher than

that of phosphorus.

a)

that the forces are stronger between sulfur (molecules) than between the phosphorus molecules

b)

there are London dispersion forces between the molecules of both these elements.These forces are stronger due to sulfur structure being S8 whereas phosphorus is P4

c)

there are London dispersion forces between the molecules of both these elements.These forces are weaker due to sulfur structure being S8 whereas phosphorus is P4

d)

that the forces are weaker between sulfur (molecules) than between the phosphorus molecules

23.

Explain the difference in polarities of ammonia and trichloramine molecules.

a)

Ammonia is polar and trichloramine is non-polar

b)

Ammonia is non-polar and trichloramine is polar

c)

Ammonia contains hydrogen bonds making it polar & the electronegativity difference in ammonia is higher than in trichloramine

d)

Ammonia contains hydrogen bonds making it non-polar & the electronegativity difference in ammonia is lower than in trichloramine

24.

Explain why covalent radius decreases across the period from

sodium to chlorine. (1) = The electron shells are pulled 1 closer because

(a)  

25.

Explain fully why the covalent radius of sodium is larger than the ionic radius of sodium.

4 lines
26.

Phosphine (PH3) is used as an insecticide in the storage of grain.State the type of bonding and structure in phosphine

a)

Covalent molecular

b)

Hydrogen

c)

Ionic

27.

State what is meant by the term electronegativity.

(a)  

28.

Covalent radius

a)

Increases down a group, decreases across a period

b)

Increases down a group, increases across a period

c)

Decreases down a group, decreases across a period

d)

Decreases down a group, increases across a period

29.

ionisation energy

a)

Increases down a group, decreases across a period

b)

Increases down a group, increases across a period

c)

Decreases down a group, decreases across a period

d)

Decreases down a group, increases across a period

30.

Electronegativity

a)

Increases down a group, decreases across a period

b)

Increases down a group, increases across a period

c)

Decreases down a group, decreases across a period

d)

Decreases down a group, increases across a period

31.

Covalent radius increases down a group because

a)

Increased number of occupied electron shells

b)

Increased positive nuclear charge

c)

Increased screening effect

d)

Decreased atomic size

e)

Increased covalent radius

32.

Covalent radius decreases across a period because

a)

Increased number of occupied electron shells

b)

Increased positive nuclear charge

c)

Increased screening effect

d)

Decreased atomic size

e)

Increased covalent radius

33.

Ionisation energy increases across a period because

a)

Increased number of occupied electron shells

b)

Increased positive nuclear charge

c)

Increased screening effect

d)

Decreased atomic size

e)

Increased covalent radius

34.

Ionisation energy decreases down a group because

a)

Increased number of occupied electron shells

b)

Increased positive nuclear charge

c)

Increased screening effect

d)

Decreased atomic size

e)

Increased covalent radius

35.

Electronegatvity decreases down a group because

a)

Increased number of occupied electron shells

b)

Increased positive nuclear charge

c)

Increased screening effect

d)

Decreased atomic size

e)

Increased covalent radius

36.

Electronegatvity increases across a period because

a)

Increased number of occupied electron shells

b)

Increased positive nuclear charge

c)

Increased screening effect

d)

Decreased atomic size

e)

Increased covalent radius

37.

What elements would have the most ionic character

a)

Biggest difference in electronegativey

b)

Smallest difference in electronegativey

38.

LDFs are

a)

Forces of attraction between all atoms and molecules as a result of electrostatic attraction between temporary dipoles and induced dipoles

b)

Additional electrostatic forces of attraction between polar molecules

c)

Electrostatic forces of attraction between molecules that contain highly polar bonds

39.

permanent dipole- permanent dipole are

a)

Forces of attraction between all atoms and molecules as a result of electrostatic attraction between temporary dipoles and induced dipoles

b)

Additional electrostatic forces of attraction between polar molecules

c)

Electrostatic forces of attraction between molecules that contain highly polar bonds

40.

Hydrogen bonding is

a)

Forces of attraction between all atoms and molecules as a result of electrostatic attraction between temporary dipoles and induced dipoles

b)

Additional electrostatic forces of attraction between polar molecules

c)

Electrostatic forces of attraction between molecules that contain highly polar bonds

41.

Why is ice less dense than water

(a)  

42.

When looking at melting and boiling point you look at..

a)

Type of van der vaal

b)

Number of electrons

c)

Hydrogen bonding

d)

If they have similar intermolecular forces

43.

When looking at viscosity you look at..

a)

Type of van der vaal

b)

Number of electrons

c)

Hydrogen bonding

d)

If they have similar intermolecular forces

44.

When looking at solubility you look at..

a)

Type of van der vaal

b)

Number of electrons

c)

Hydrogen bonding

d)

If they have similar intermolecular forces

45.

The anomalous bp of ammonia, water & hydrogen fluoride is a result of

a)

Hydrogen bonding

b)

LDP

c)

Ionic bonding

d)

Covalent lattice

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