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Atomic Structure and Period Table Test Review

Total questions: 58

Worksheet time: 2hrs 44mins

Name
Class
Date
1.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
2.
Who arranged the periodic table by increasing atomic number?
a)
Mendeleev
b)
Rutherford
c)
Bohr
d)
Mosely
3.
What was Dmitri Mendeleev's greatest contribution to the history of the periodic table?
a)
He arranged all of the known elements by their atomic number
b)
He realised that there was a pattern of reactivity which repeated every 8 elements
c)
He predicted the existence (and properties) of new elements
d)
He identified the "law of triads" which became the groups
4.

Which of the following are found in the nucleus?

a)

protons and electrons

b)

protons ONLY

c)

protons and neutrons

d)

Electrons only

5.

_________________________ are the rows on the periodic table while _______________________ are the columns.

a)

periods/ groups(families)

b)

groups(families)/periods

c)

metals/non-metals

d)

non-metals/metals

6.

Which of the following elements is in (period 4 , group 2)

a)

Carbon

b)

Potassium

c)

Calcium

d)

Sodium

7.
What element is will have the most similar physical and chemical properties to the element Lithium (Li)?
a)
Sodium (Na)
b)
Magnesium (Mg)
c)
Beryllium (Be)
d)
Calcium (Ca)
8.
Elements which are shiny, conduct electricity and heat are called
a)
metal
b)
nonmetal
c)
metalloid
d)
nonexistent
9.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
10.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
11.

The atomic radius across period

a)

decrease from left to right

b)

Increase from left to right

c)

decrease from right to left

d)

stay the same

12.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
13.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
14.

What subatomic particle does not contribute to mass?

a)

Protons

b)

Neutrons

c)

Electrons

15.

What is the identity of the atom?

a)

Aluminum

b)

Silicon

c)

Cobalt

d)

Zirconium

16.

Which is the best nuclear symbol for a potassium atom with 21 neutrons?

a)
b)
c)
d)
17.

What is the ionic charge of this atom?

a)

-2

b)

-1

c)

+1

d)

+2

18.

What is the chemical symbol for an element with 21 protons and 19 electrons?

a)

K2+K^{2+}  

b)

KK  

c)

  Sc2+Sc^{2+}  

d)

Sc2−Sc^{2-}  

19.

Why do the electrons surround the nucleus?

a)

the negative electrons are attracted to the neutral neutrons

b)

the negative electrons are repelled by the neutral neutrons

c)

the negative electrons are attracted to the positive protons

d)

the negative electrons are repelled by the positive protons

20.
Carbon-12, Carbon-13, and Carbon-14 are...
a)
ions
b)
isotopes
c)
electronegative
d)
radioactive
21.

The Lanthanide and Actinide series of elements are known as the:

a)

Common earth metals

b)

Alkaline earth metals

c)

Rare earth metals

d)

Heavy earth metals

22.

What is the configuration for Carbon?

a)

1s2 2p2

b)

1s2 2s2 2p2

c)

1s1 1s2 2s2 2p2

23.

Which element is 1s2 2s2 2p6 3s2 3p6 4s2 3d7?

a)

Cobalt

b)

Nickel

c)

Manganese

d)

Chromium

24.

Which of the following will have similar properties to 1s2 2s2 2p6 3s2 3p2?

a)

carbon

b)

calcium

c)

chlorine

d)

cesium

25.

What is the position of an element in the periodic table if its electron configuration is 1s2 2s2 2p6 3s2 3p5?

a)

Group 1A

b)

Group 2A

c)

Group 5A

d)

Group 7A

26.

What is the noble gas notation electron for Sulfur?

a)

[Ne] 3p4

b)

[He] 3s2 3p4

c)

[Ne] 3s2 3p4

d)

[Na] 3s2 3p4

27.

What is the noble gas configuration for silicon?

a)

[Ne] 3s2 3p1

b)

[Ar] 4s1

c)

[Kr] 5s1

d)

[Ne] 3s2 3p2

28.
Question Image

Match the parts of the electron configuration to what it represents.

a)

1

1.

period

b)

s

2.

block

c)

2

3.

element

29.

Match the group to the configuration that it ends with.

a)

s1

1.

alkali metals

b)

s2

2.

alkaline earth metals

c)

p5

3.

halogens

d)

p6

4.

noble gases

30.

What is the missing piece?

1s2 2s2 ___ 3s1

a)

2p6

b)

2p4

c)

3p6

d)

3s2

31.

Match the element to it's noble gas notation:

a)

krypton

1.

[Kr]

b)

silicon

2.

[Ne] 3s2 3p2

c)

strontium

3.

[Kr] 5s2

d)

copper

4.

[Ar] 4s2 3d9

32.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
33.
How many total electrons can the f orbitals in a sublevel hold?
a)
2
b)
14
c)
6
d)
10
34.
Electrons are paired based on their spin directions, clockwise and counterclockwise, is what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
35.

Which orbital shows a violation of Hund's Rule?

a)

A

b)

B

c)

C

d)

D

e)

None of these

36.

Which orbital shows a violation of the Pauli Exclusion Principle?

a)

A

b)

B

c)

C

d)

D

e)

None of these

37.

Which orbital shows a violation of the Aufbau Principle?

a)

A

b)

B

c)

C

d)

D

e)

None of these

38.

What is incorrect about this orbital diagram?

a)

Both arrows in the 2p box should be pointing up

b)

Nothing

c)

One of the electrons in the first 2p box should be placed in the second 2p box, still pointing down

d)

One of the electrons in the first 2p box should be placed in the second 2p box, pointing up

39.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
40.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
41.
This is the correct dot diagram for nitrogen (N)
a)
true
b)
false
42.

What is the electron configuration of sodium ion (Na+1)?

a)

2-8

b)

2-8-2

c)

2-8-1

d)

11

43.
How many valence electrons are in an atom of Ar?
a)
2
b)
8
c)
4
d)
1
44.

Light is emitted when electrons ...

a)

return from high energy state to low energy state

b)

jump from low energy state to high energy state

c)

either of these

d)

none of these

45.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Helium

46.
 The diagram above represents two electrons with 
a)
a. opposite spins.
b)
 b. the same spin.
c)
c. different energies.
d)
d. different energy levels.
47.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
48.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
49.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
50.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

51.

What is a positively-charged ion which forms when an atom loses electrons?

a)

atom

b)

ion

c)

cation

d)

anion

52.

As you move across a period, what happens to the nuclear charge in the atoms?

a)

It increases because more protons are added.

b)

It decreases because protons are taken away.

c)

It stays the same.

53.

What idea is this cartoon showing?

a)

chlorine is more electronegative than hydrogen

b)

chlorine has more energy levels than hydrogen

c)

hydrogen is more electronegative than chlorine

54.

The atom is mostly large empty space with a small, dense nucleus at the center

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

55.

Atoms are indivisible (cannot be broken down)

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

56.

In a famous experiment conducted by Ernest Rutherford, positively charged alpha particles were scattered by a thin gold foil. Which of the following is a conclusion that resulted from this experiment?

a)

The nucleus is negatively charged

b)

The atom is a dense solid and is indivisible

c)

The mass is conserved when atoms react chemically

d)

The nucleus is very small and the atom is mostly empty space

57.
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
58.
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.
How many protons does this element have?
a)
32
b)
33
c)
34
d)
no way to know

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