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Atomic structure and bonding revision

Total questions: 33

Worksheet time: 3hrs 25mins

Name
Class
Date
1.

Ionisation energy is ___________.

a)

maximum energy required to remove 1 electron from 1 mol of gaseous atom

b)

minimum energy required to remove 1 electron from 1 mol of gaseous atom

c)

first ionisation energy

d)

second ionisation energy

2.

When across a period, the atomic size decreases so the first IE ___________.

a)

increases

b)

decreases

c)

constant

d)

i am not sure

3.

When going down a group, the atomic size increases so the first IE __________.

a)

increases

b)

decreases

c)

constant

d)

I am not sure

4.

The equation for the first ionisation energy of a sodium atom is:

a)

Na (g) -> Na+ (g) + e-

b)

Na+ (g) -> Na2+ (g) + e-

c)

Na (s) -> Na+ (g) + e-

d)

Na+ (g) + e- -> Na (g)

5.

Which of the following has a lowest first ionisation energy?

a)

Sodium (Na)

b)

Magnesium (Mg)

c)

Chlorine (Cl)

d)

Argon (Ar)

6.

Which has the lower first ionisation energy between magnesium and aluminium elements and why

a)

Magnesium because it has a lower nuclear charge and higher atomic radius

b)

Aluminium because it has fewer protons

c)

Magnesium because its outermost electron is removed from an orbital further from the nucleus

d)

Aluminium because it is removed from an orbital which is higher in energy

7.

Which is the correct statement? (IE = ionisation energy)

a)

Magnesium has a higher FIRST IE than sodium because it wants to lose 2 electrons not one.

b)

Sulfur has a lower first IE than phosphorus because of repulsion between paired electrons in the 3p subshell.

c)

Sulfur has a lower first IE than phosphorus because of repulsion between paired electrons in the 2p subshell.

d)

First IE energy decreases across a period as the atoms get bigger

8.

Which one is a correct statement? (IE = FIRST ionisation energy)

a)

13Al has a lower IE than 14Mg because Al has fewer protons

b)

13Al has a lower IE than 14Mg because Al has electron in 3p subshell which is higher energy and shielded.

c)

13Al has a lower IE than 14Mg because Al has a pair of electrons repelling in 3p subshell.

d)

13Al has a lower IE than 14Mg because Al has a larger atomic radius.

9.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
10.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
11.

How many electron can be found in a p orbital?

a)

2

b)

3

c)

4

d)

6

12.
24.1% of all the isotopes of a an element have a mass of 75.23 amu, 48.7% have a mass of 74.61 amu, and 27.2% have a mass of 75.20 amu.
What is the average mass of this element?
a)
74.92 amu
b)
24.97 amu
c)
75.01 amu
d)
74.51 amu
13.
4.35% of all X atoms have a mass of 39.946 amu. 83.79% have a mass of 41.941 amu, 9.50% have a mass of 42.941 amu, and 2.36% have a mass of 43.939 amu. What is the average atomic mass of atom X?
a)
41.97 amu
b)
42.19 amu
c)
10.43 amu
d)
40.04 amu
14.

Which of the following molecules does NOT have a linear shape?

a)

CS2

b)

HCN

c)

OF2

d)

BeF2

15.

In which of the following pairs, do the molecules have a similar shape?

a)

BeCl2 and Cl2O

b)

SCl2 and CO2

c)

BF3 and NH3

d)

BH3 and CH2O

16.

Which species has a shape that is influenced by the presence of one or more lone pairs of electrons around the central atom?

a)

AlCl3

b)

ClF3

c)

IF6+

d)

PCl6–

17.

Which species has one or more bond angle(s) of 90°?

a)

CH4

b)

NH4+

c)

ClF4−

d)

AlCl4−

18.

Which of these species has a trigonal planar structure?

a)

PH3

b)

BCl3

c)

H3O+

d)

CH3−

19.

Which one of the following is the most likely value for the bond angle α shown in the diagram of SF4?

a)

118°

b)

101°

c)

90°

d)

88°

20.

Which of the following compounds consists of dipole molecules?

a)

H2S

b)

CH4

c)

CO2

d)

N2

21.

Which statement explains why Br2 is a liquid at STP and I2 is a solid at STP?

a)

Molecules of Br2 are polar, and molecules of I2 are nonpolar

b)

Molecules of Br2 are nonpolar, and molecules of I2 are polar

c)

Molecules of Br2 have stronger intermolecular forces than molecules of I2.

d)

Molecules of I2 have stronger intermolecular forces than molecules of Br2.

22.

In which molecule is hydrogen bonding the strongest?

a)

HF

b)

HCl

c)

HBr

d)

HI

23.

The correct ranking of intermolecular forces in order of greatest to least

a)

dipole-dipole, Hydrogen bonding, van der Waal forces

b)

van der Waal forces, hydrogen bonding, dipole-dipole attraction

c)

Hydrogen bonding, dipole-dipole attraction, van der Waals forces

d)

van der waal forces, dipole-dipole attractions, Hydrogen bonding

24.

The attraction that exists between carbon dioxide molecules in solid carbon dioxide is due to

a)

covalent bonding

b)

Hydrogen bonding

c)

dipole-dipole attractions

d)

van der Waal forces

25.

All intermolecular forces involve...

a)

bonding by sharing electrons

b)

bonding by transferring electrons

c)

hydrogen atoms that are involved in a bond

d)

slightly positive and slightly negative poles

26.
Giant lattice structure held together by attraction between  positive and negatively charged ions 
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
27.
Elements such as  Silicon, diamond and graphite.  Compounds include  SiO2
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
28.

The bond created by the electrostatic attraction between metal cations and delocalised valence electrons

a)

Hydrogen bonding

b)

Covalent bonding

c)

London forces

d)

Dipole-dipole forces

e)

Metallic bonding

29.

The bond created by the electrostatic attraction between metal cations and non-metal anions

a)

Hydrogen bonding

b)

Covalent bonding

c)

Ionic Bonding

d)

Dipole-dipole forces

e)

Metallic bonding

30.

The bond created when the difference in electronegativity between two atoms is greater than 1.8

a)

Hydrogen bond

b)

Non-polar covalent bond

c)

Ionic bond

d)

Polar covalent bond

e)

Metallic bond

31.

The bond created when the difference in electronegativity between two atoms is less than 1.8 but not zero

a)

Hydrogen bond

b)

Non-polar covalent bond

c)

Ionic bond

d)

Polar covalent bond

e)

Metallic bond

32.

The bond created when the difference in electronegativity between two atoms is zero

a)

Hydrogen bond

b)

Non-polar covalent bond

c)

Ionic bond

d)

Polar covalent bond

e)

Metallic bond

33.

The dominant type of intermolecular attractions between polar molecules

a)

Hydrogen bonding

b)

Covalent bonding

c)

London forces

d)

Dipole-dipole forces

e)

Metallic bonding

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