Wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Final exam review Unit 2 - Atomic theory + Electronic config

Total questions: 69

Worksheet time: 1hrs 13mins

Name
Class
Date
1.
J.J. Thomson provided evidence that an atom...
a)
is the smallest particle of matter
b)
contains negatively charged particles
c)
has an overall negative charge
d)
has an overall positive charge
2.
Rutherford discovered the...
a)
electron
b)
proton
c)
neutron
d)
nucleus
3.
Isotopes are elements with a different amount of
a)
protons
b)
neutrons
c)
electrons
d)
atoms
4.
an element will always have the same number of 
a)
neutrons
b)
protons
c)
isotopes
d)
atoms
5.
Which particle does not contribute mass to the atom?
a)
Proton
b)
Neutron
c)
Electron
d)
Nucleus
6.
What scientist is best known for his gold foil experiment?
a)
J.J. Tomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
7.
An atom has 10 protons and a mass of 18. It has __ neutrons
a)
10
b)
18
c)
28
d)
8
8.
An ______________ is the same element, with the same number of protons, but different numbers of neutrons
a)
Atom
b)
Isotope
c)
Atomic Number
d)
Mass Number
9.
The smallest particle into which an element can be divided and still be the same substance
a)
neutron
b)
atom
c)
electron
10.
The mass number of an element that has18 protons, 18 electrons, and 19 neutrons is _____.
a)
12.5
b)
13
c)
25
d)
37
11.
How many neutrons does uranium-239 have
a)
92
b)
147
c)
239
d)
331
12.
How many neutrons will an atom have it has an atomic number of 26, an atomic mass of 58 and a charge of +3?
a)
26
b)
58
c)
32
d)
3
13.
How many electrons are in an atom that has an atomic number of 34, an atomic mass of 74 and a charge of -2?
a)
34
b)
36
c)
2
d)
40
14.
How many protons are in an atom with an atomic number of 20, an atomic mass of 45, and a charge of +2?
a)
20
b)
10
c)
2
d)
18
15.
What charge does an atom have if it GAINS an electrons?
a)
Positive (+)
b)
Negative (-)
16.

The electron configuration of an atom is 1s22s22p61s^22s^22p^6 The number of electrons in the atom is 

a)

3

b)

5

c)

6

d)

10

17.

What is the Aufbau principle?

a)

Within an energy level, s orbitals are the lowest energy, followed by p, d and then f. F orbitals are the highest energy for that level.

b)

All three.

c)

The lower the principal quantum number (n) the lower the energy.

d)

The Aufbau Principle states that electrons enter the lowest energy orbitals first.

18.

Which one of the following is the electronic configuration of the bromine atom?

a)

1s22s22p63s23p63d104s14p6

b)

1s22s22p63s23p63d104s24p7

c)

1s22s22p63s23p63d104s24p5

d)

1s22s22p63s23p63d104s24p6

19.

Which one of the following does not represent the electronic configuration of an atom in its ground state?

a)

1s2 2s2 2p3

b)

1s2 2s2 2p4

c)

1s2 2s2 2p6 3s1

d)

1s2 2s2 2p6 3d1

20.

Which one of the following contains no unpaired electrons in the ground state?

a)

Be

b)

F

c)

Si

d)

N

21.

Which one of the following is the electronic structure of a metal with a maximum oxidation state of +3?

a)

1s2 2s2 2p6 3s1

b)

1s2 2s2 2p6 3s2 3p4

c)

1s2 2s2 2p6 3s2 3p1

d)

1s2 2s2 2p6 3s2 3p6 3d10 4s2

22.

The number of electrons in the 3d orbital of the atom of atomic number 27 is

a)

5

b)

6

c)

7

d)

10

23.

The vanadium atom (atomic number 23) in its ground state has the electronic configuration:

a)

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

b)

1s2 2s2 2p6 3s2 3p6 3d2 4s3

c)

1s2 2s2 2p6 3s2 3p6 3d1 4s2 4p2

d)

1s2 2s2 2p6 3s2 3p6 3d2 4s2 4p1

24.
What is the noble gas shorthand electron for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p4
25.
What is the electron configuration for this atom?
a)
1s22s22p6
b)
1s22s22p5
c)
1s22s22p3
d)
2s22p3
26.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
27.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
28.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
29.
What is the electronic configuration of sodium?
a)
1s22s22p63s1
b)
[Ne]3s1
c)
1s22s22p7
d)
Both A and B are correct
30.
What is the electronic configuration of iron?
a)
1s22s22p63s23p64s23d6
b)
1s22s22p63s23p63d8
c)
1s22p63s23p64s23d6
d)
1s22s22p63s23p64s13d6
31.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)

1s22s22p4

c)
1s22s22p6
d)
1s22s22p63s23p6
32.

The Aufbau principle states:

a)

lower energy orbitals fill before higher energy orbitals

b)

one electron goes into each until all of them are half full before pairing up.

c)

no two electrons can be identified by the same set of quantum numbers (i.e. must have different spins).

d)

the position and the velocity of an electron cannot both be measured exactly, at the same time, even in theory.

33.

Hunds rule states:

a)

lower energy orbitals fill before higher energy orbitals

b)

one electron goes into each orbital until all of them are half full before pairing up.

c)

no two electrons can be identified by the same set of quantum numbers (i.e. must have different spins).

d)

the position and the velocity of an electron cannot both be measured exactly, at the same time, even in theory.

34.

Pauli's exclusion principle states:

a)

lower energy orbitals fill before higher energy orbitals

b)

one electron goes into each orbital until all of them are half full before pairing up.

c)

no two electrons can be identified by the same set of quantum numbers (i.e. must have different spins).

d)

the position and the velocity of an electron cannot both be measured exactly, at the same time, even in theory.

35.

Copper has which of the following electron configurations?

a)

1s2 2s2 2p6 3s2 3p6 3d10 4s1

b)

1s2 2s2 2p6 3s2 3p6 3d9 4s2

c)

1s2 2s2 2p6 3s2 3p6 3d7 4s2 4p2

d)

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

36.

Fe3+ ions have which electron arrangement?

a)

1s2 2s2 2p6 3s2 3p6 3d6 4s2

b)

1s2 2s2 2p6 3s2 3p6 3d5

c)

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

d)

1s2 2s2 2p6 3s2 3p6 3d4 4s1

37.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
38.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
39.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
40.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
41.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
42.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
43.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
44.
The energy required to remove electrons is the definition of: 
a)
Electronegativity
b)
Atomic Number
c)
Atomic Radius
d)
Ionization
45.
What is the name of family I
a)
Alkaline Earth Metals
b)
Boron Family
c)
Alkali Metals
d)
Halogen Family
46.
Group B is known as the:
a)
Inner Metals
b)
Transition Metals
c)
Weirdos
d)
Changelings 
47.
Families all have similar 
a)
Names
b)
atomic numbers
c)
atomic masses
d)
properties
48.
Electronegativity is...
a)
the ability of an atom to attract/ accept 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. 
49.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
50.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
51.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
52.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
53.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
54.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

55.

Which of the following will have a higher electronegativity than arsenic (As)?

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

56.

Which of the following halogens has the greatest electronegativity?

a)

Chlorine (Cl)

b)

Bromine (Br)

c)

Iodine (I)

d)

Astatine (At)

57.

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

a)

atom

b)

ion

c)

cation

d)

anion

58.

What is a negatively-charged ion which forms when an atom gains electrons?

a)

cation

b)

anion

c)

electron

d)

ion

59.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
60.

Atomic radius INCREASES when you go (a)   a group

61.

Put in order from biggest to smallest (decreasing size)

a)

Calcium

b)

Iron

c)

Zinc

d)

Bromine

e)

Krypton

1)
2)
3)
4)
5)
62.

Which of the following atoms would have the largest radius?

a)

chlorine

b)

silicon

c)

sodium

d)

argon

63.

Why does radius decrease as you move across a period?

a)

because electrons are being added

b)

because protons are being added

c)

because energy levels are being lost

d)

because energy levels are being added

64.

Which of the following has the largest electronegativity value?

a)

neon

b)

fluorine

c)

carbon

d)

lithium

65.

Which has the greater electronegativity Cl or Al?

a)
Cl
b)
Al
66.
How are elements on the periodic table arranged by?
a)
in alphabetic order
b)
simular physical & chemical properties
c)
their symbols
d)
Just simular physical properties
67.

Which element in Period 3 has the highest electronegativity?

a)

Sodium (Na)

b)

Chlorine (Cl)

c)

Aluminum (Al)

d)

Argon (Ar)

68.

As you move across a period, which of the following properties generally increases?

a)

Atomic radius

b)

Electronegativity

c)

Metallic character

d)

Number of energy levels

69.

Which of the following elements has the smallest atomic radius in Group 1?

a)

Hydrogen (H)

b)

Lithium (Li)

c)

Sodium (Na)

d)

Potassium (K)

Similar Resources on Wayground

Solving and Graphing Linear and Absolute Value Inequalities

69 questions

Solving and Graphing Linear and Absolute Value Inequalities

quiz

Worksheet

•

9th - 12th Grade

Honors Algebra 1 Semester Review

70 questions

Honors Algebra 1 Semester Review

quiz

Worksheet

•

9th - 12th Grade

Unit 9 Functions and Slope Review

64 questions

Unit 9 Functions and Slope Review

quiz

Worksheet

•

8th - 10th Grade

Geometry Review Day 2

70 questions

Geometry Review Day 2

quiz

Worksheet

•

9th - 10th Grade

AP Statistics Semester 1 Review

65 questions

AP Statistics Semester 1 Review

quiz

Worksheet

•

9th - 12th Grade

Unit 8AB Review

64 questions

Unit 8AB Review

quiz

Worksheet

•

8th - 10th Grade

Algebra 1A Final Exam Review

65 questions

Algebra 1A Final Exam Review

quiz

Worksheet

•

9th - 10th Grade

Maths challenge fun

65 questions

Maths challenge fun

quiz

Worksheet

•

8th Grade - University