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IB Chemistry Chapter 2 - Atomic Theory

Total questions: 60

Worksheet time: 1hrs 9mins

Name
Class
Date
1.

Which of the following elements has the lowest first ionization energy?

a)

Argon

b)

Magnesium

c)

Sodium

d)

Lithium

2.

John Dalton stated:

a)

Atoms are tiny, invisible particles.

b)

Atoms of one element are all the same.

c)

Atoms of different elements are different.

d)

Compounds form by combining atoms.

e)

All of the statements listed.

3.
The word "atom" comes from a Greek word that means
a)
Invisible
b)
Indivisible
c)
Undivided
4.
Place the following scientists in order, from earliest to latest: 
Rutherford, Dalton, Bohr, Thomson
a)
Dalton, Rutherford, Bohr, Thomson
b)
Thomson, Dalton, Rutherford, Bohr
c)
Dalton, Thomson, Rutherford, Bohr
d)
Bohr, Dalton, Rutherford, Thomson
5.

Which orbitals cannot exist

a)

3p

b)

4d

c)

3f

d)

6s

6.

Light is emitted when an electron moves from the ________ state to the _________ state.

a)

excited, ground

b)

ground, excited

7.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

8.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
9.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
10.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
11.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
12.
Which orbital shows a violation of the Aufbau Principle?
a)
A
b)
B
c)
C
d)
D
13.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
14.
Which of the following statements is true about the 3s and the 4s sublevels?
a)
These sublevels have the same energy
b)
These sublevels are the same distance from the nucleus
c)
These sublevels hold different amounts of electrons
d)
These sublevels have the same shape
15.
The graph above shows the ionization energy values as the elements are arranged on the periodic table. Which conclusion cannot be drawn from the graph?
a)
The ionization energy drops significantly as you move down a group because the valence electrons are in a shell further from the nucleus.
b)
The ionization energy increases gradually as you move right across a period because the valence electrons are in a shell further from the nucleus.
c)
The ionization energy increases gradually as you move right across a period because you are adding more protons.
d)
The ionization energy increases when the valence electrons are more attracted to the nucleus.
16.
The bar graph above represents four elements and their respective ionization energies. Based on the organization of the modern periodic table, how would these elements be found on the periodic table?
a)
They are in the same period with W being furthest left.
b)
They are in the same period with W being furthest right.
c)
They are in the same group with W being furthest to the bottom.
d)
They are in a diagonal line with W being at the bottom right.
17.
Which of the following sequences corresponds to a correct trend in ionization energy?
a)
Cl > S > P > Al
b)
Sr > Ca > Mg > Be
c)
Rb > K > Na > Li
d)
Rb > Sr > I > Xe
18.
Put the following in order of increasing ionization energy:Neon, Lithium, Carbon
a)
Lithium, Carbon, Neon
b)
Carbon, Lithium, Neon
c)
Neon, Carbon, Lithium
d)
Lithium, Neon, Carbon
19.
Put the following in order of increasing ionization energy:Cobalt, Tungsten, Ruthenium
a)
Tungsten, Ruthenium, Cobalt
b)
Cobalt, Tungsten, Ruthenium
c)
Ruthenium, Cobalt, Tungsten
d)
Cobalt, Ruthenium, Tungsten
20.

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

21.

Which equation correctly describes the first ionization energy of X?

a)

X --> X- + e-

b)

X --> X+ + e-

c)

X --> X- + e+

d)

X + e- --> X-

e)

X + e- --> X+

22.

Successive ionization energies for an element in Period 4 were determined experimentally and found to be: IE1=600 kJ/mol, IE2=1800 kJ/mol, IE3=2700 kJ/mol, IE4=11,600 kJ/mol and IE5=15,000 kJ/mol. What element is this?

a)

germanium

b)

selenium

c)

gallium

d)

silicon

e)

phosphorous

23.

Using electron configuration and your knowledge of ionization energy, which would you expect to have a higher second ionization energy: Na or Mg?

a)

Na

b)

Mg

c)

Both would be expected to have the same second ionization energy

d)

Cannot be determined

24.

Which statement best describes the relative first ionization energies of Ca and Mg?

a)

Calcium has a higher first ionization energy than magnesium because its radius is smaller.

b)

Magnesium has a higher first ionization energy than calcium because its radius is smaller.

c)

Calcium has a higher first ionization energy than magnesium because its highest occupied energy sub-level is full.

d)

Magnesium has a higher first ionization energy than calcium because its highest occupied energy sub-level is full.

e)

Calcium and magnesium will have the same first ionization energy because they have the same number of valence electrons.

25.

What is the wavelength of red light (in nm) with a frequency of 4.55 x 1014 Hz?

a)

659 nm

b)

1.52 x 106 nm

c)

455 nm

d)

152 nm

e)

none of these

26.

The four lines observed in the emission spectrum of hydrogen tell us that ___.

a)

The hydrogen molecule has the formula H4.

b)

We could observe more lines if we had a stronger prism.

c)

There are four electrons in an excited hydrogen atom.

d)

There are four allowable energy jumps for the electron in a hydrogen atom.

e)

The spectrum of hydrogen is continuous.

27.

Which one of the following types of electromagnetic radiation will travel at the highest speed?

a)

gamma radiation

b)

ultraviolet (UV) radiation

c)

infrared (IR) radiation

d)

visible light

e)

None of these

28.

If an electron in the hydrogen atom falls from n=5 to n=2, is this emission or absorption?

a)

emission

b)

absorption

c)

both emission and absorption

d)

neither emission or absorption

29.
a)

A

b)

B

c)

C

d)

D

30.
a)

a

b)

b

c)

c

d)

d

31.
a)

A

b)

B

c)

C

d)

D

32.
a)

a

b)

b

c)

c

d)

d

33.
Which species would get deflected by the greatest degree in the mass spectrometer?
a)
12C+
b)
13C+
c)
13C2+
d)
14C+
34.
What do the peaks on the mass spectrum represent?
a)
anions
b)
different isotopes
c)
atoms with differing numbers of electrons
d)
numbers of electrons
35.
What do the heights of the peaks represent in the mass spectrum?
a)
number of isotopes
b)
relative abundance of each isotope
c)
average atomic mass
d)
charge:mass ratio
36.
How many isotopes are shown in this mass spectrum?
a)
1
b)
84
c)
86
d)
4
37.
Based on the mass spectrum, which isotope of chlorine is most abundant?
a)
35Cl
b)
37Cl
c)
70Cl
d)
72Cl
38.
Use your periodic table.  There are two isotopes of rubidium: 85Rb and 87 Rb. Which is more abundant?
a)
equally abundant
b)
rubidium-85
c)
rubidium-85.47
d)
rubidium-87
39.
What is the average atomic mass for this element?
a)
10 amu
b)
10.8 amu
c)
19.9 amu
d)
11 amu
40.
The average atomic mass rhenium, Re, is 186.21 amu. If 37.1% of rhenium has mass# = 185, what is the other stable isotope?
a)
Rhenium-183
b)
Rhenium-181
c)
Rhenium-187
d)
Rhenium-189
41.
What are the steps of operation in the mass spectrometer?
a)
Accelerate, Deflect,Ionize, Detect
b)
Deflect,Ionize, Accelerate, Detect
c)
Ionize, Accelerate, Deflect, Detect
d)
Detect, Accelerate, Deflect, Ionize
42.
What is the average atomic mass for this element?
a)
10 amu
b)
10.8 amu
c)
19.9 amu
d)
11 amu
43.
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
44.

Lithium has an elemental atomic mass of 6.941 amu and has two naturally occurring isotopes, 6Li and 7Li. Their masses are 6.0151 amu and 7.0160 amu respectively. What are the percentage abundances for each isotopes of Lithium?

a)

6Li = 7.49% 7Li = 92.51%

b)

6Li = 10.61% 7Li = 89.39%

c)

6Li = 40.20% 7Li = 59.80%

d)

6Li = 70% 7Li = 30%

45.

This orbital diagram represents

a)

Nitrogen

b)

Oxygen

c)

Carbon

d)

Neon

46.

With what neutral element is Ag+ isoelectronic?

a)

Cd

b)

Pd

c)

Xe

d)

Kr

47.

A shorter atomic radius of atoms in the same period will result in:

a)

A higher first ionisation energy

b)

A lower first ionisation energy

48.

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

49.

*The first three successive ionisation energies for the element N increase gradually but the fourth ionisation energy increases sharply.

*Element N is a third period element.

*N form an amphoteric oxide.


Which of the following s electronic configuration matches the statements above?

a)

1s2 2s2 2p6 3s2 3p1

b)

1s2 2s2 2p6 3s2 3p3

c)

1s2 2s2 2p6 3s2 3p6 3d1 4s2

d)

1s2 2s2 2p6 3s2 3p6 3d3 4s2

50.

Based on the successive ionisation energies below,how many valence electrons does the element M have?


IE1 = 943

IE2 = 1,950

IE3 = 3,852

IE4 = 5,492

IE5 = 23,085

IE6 = 26,791

IE7 = 30,024

a)

2

b)

3

c)

4

d)

5

51.

Element Q has the following electronic configuration:

1s2 2s2 2p6 3s2 3p6 3d5 4s1


Which of the following is true about the position of element Q in periodic table?

a)

Period 3, Group 1, Block s

b)

Period 4, Group 16, Block d

c)

Period 4, Group 6, Block d

d)

Period 4, Group 1, Block s

52.

How many of each subatomic particle would you find in a Calcium ion?

a)

20 protons, 20 neutrons, 18 electrons

b)

20 protons, 40 neutrons, 18 electrons

c)

20 protons, 20 neutrons, 22 electrons

d)

20 protons, 40 neutrons, 22 electrons

53.

The line with the shortest wavelength is produced in the hydrogen spectrum when electron moves

a)

from n=2 to n=1

b)

rom n=4 to n=1

c)

from n=3 to n=1

d)

from n=4 to n=3

54.

Which type of spectra is this?

a)

Continuous

b)

Emission

c)

Absorption

55.

In an emission spectra, lines will converge towards what color?

a)

red

b)

blue

c)

green

d)

violet

56.

Which electron transition between the energy

levels of hydrogen causes the emission of a photon of

visible light?

a)

𝑛 = 6 to 𝑛 = 5

b)

𝑛 = 5 to 𝑛 = 6

c)

𝑛 = 5 to 𝑛 = 2

d)

𝑛 = 2 to 𝑛 = 5

57.

Which type of photon is emitted when an electron

in a hydrogen atom drops from the n=2 to the n=1

energy level?

a)

Ultraviolet

b)

Visible light

c)

Infrared

d)

Radio wave

58.

The visible lines from hydrogen are all members

of the ____.

a)

Lyman series

b)

Balmer series

c)

Paschen series

d)

Lyman and Paschen series

59.

An element has the elctron configuration 2.7. What would be the elctron configuration of an element with similar chemical properties?

a)

2.6

b)

2.8

c)

2.7.1

d)

2.8.7

60.

All of the following factors affect the value of the ionization energy of an atom except the...

a)

mass of the atom

b)

charge on the nucleus

c)

size of the atom

d)

main energy level from which the electron is removed

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