wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

G11 Q1 final exam revision 25-26

Total questions: 100

Worksheet time: 3hrs 17mins

Name
Class
Date
1.

Which of the following is the best evidence that the particles that make up a cathode ray had a negative charge?

a)

The particles were produced by many different metals.

b)

The ray was attracted toward a positive electric field.

c)

Line emission spectra for an element are always the same.

d)

The ray caused a phosphorescent screen to glow.

2.

What is the electrical charge of the cathode & anode respectively ?

a)

Negative & positive

b)

Positive & negative

c)

neutral & Positive

d)

unknown

3.

Which of the following sublevels can not be found in a given atom? select 3

a)

4s

b)

3f

c)

2d

d)

1p

4.

Which of the following are similar in their electric charges? select 2

a)

electron – Cathode

b)

Alpha – Atom's nucleus

c)

Cathode – Atom's nucleus

d)

Alpha – Electron

5.

If the difference of energy between 6th & 7th level is E1 so the difference between the 1st 2nd levels is …………

a)

More than E1

b)

Less than E1

c)

Equal to E1

d)

Quit more than E1

6.

Which force holds protons and neutrons together in the atom nucleus?

a)

electric force

b)

gravity

c)

strong nuclear force

d)

weak nuclear force

7.

Mass defect is ..

a)

the sum of parent particles and daughter particles

b)

the difference of mass of parent particles and daughter particles

c)

the sum of daughter particles

d)

the sum of parent particles

8.

Which type of decay is a type of wave?

a)

alpha

b)

beta

c)

gamma

9.

Bohr's atomic model differs from that of Rutherford, this difference is obvious in Bohr’s postulate that the electron ............

a)

is a negatively charged particle.

b)

revolves around the nucleus in certain orbits.

c)

produces a spectral line when it loses a quantum.

d)

does not produce a spectral line when it loses a quantum.

10.

According to Bohr’s atomic model, the electron, ..... to transfer from the first level K to the fourth level N

a)

acquires a quantum

b)

acquires 4 quanta

c)

loses 4 quanta

d)

loses a quantum

11.

The shape of the s sub level

a)

spherical

b)

dumb bell

c)

triangular

12.

What's a valence electron?

a)

the atomic number

b)

electrons in the second energy level

c)

electrons in the first level

d)

electrons in the outermost energy level

13.

If an electron moves from lower energy level to higher energy level it is called

a)

excited state

b)

ground state

c)

neutral state

14.

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

a)

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

b)

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

c)

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

d)

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

15.

If an electron moves from n=5 to n=2 ...

a)

it releases energy

b)

it absorbs energy

16.

What is the shape of 'p' orbitals?

a)

Dumbbell shaped

b)

Spherical shaped

c)

Hybrid structure

d)

Peanut shaped

17.

How many orbitals in the f-orbital?

a)

3

b)

5

c)

7

d)

1

18.

For an electron to change from ground state to an excited stated it must...

a)

Absorb energy

b)

Release energy

19.

How many electrons can the s sublevel hold?

a)

2

b)

6

c)

14

d)

10

20.

What are the orbitals for n=4

a)

s, p

b)

s, p, d

c)

s

d)

s, p, d, f

21.

Who Proposed that electrons can jump between energy levels?

a)

Plank

b)

DeBrogile

c)

Milliken

d)

Bohr

22.

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

a)

1s2 2s2 2p6 3s11s^2\ 2s^2\ 2p^6\ 3s^1

b)

1s2 2s2 2p6 3d11s^2\ 2s^2\ 2p^6\ 3d^1

c)

1s2 2s2 2p31s^2\ 2s^2\ 2p^3

d)

1s2 2s2 2p41s^2\ 2s^2\ 2p^4

23.

The amount of energy required to move electron from one energy level to other

a)

quantum

b)

photon

c)

ATP

24.

The electron configuration of an atom is 1s2 2s2 2p61s^2\ 2s^2\ 2p^6 The number of electrons in the atom is

a)

5

b)

3

c)

6

d)

10

25.

The number of electrons in the 3d orbital of the atom of atomic number 24 is

a)

7

b)

10

c)

4

d)

5

26.

How many electrons can the d sublevel hold?

a)

2

b)

14

c)

10

d)

6

27.

If an electron moves from n=2 to n=4 ...

a)

it releases energy

b)

it absorbs energy

28.

The atomic sublevel with the next highest energy after 4p is

a)

5p

b)

4d

c)

5s

d)

4f

29.

electronic configuration of ion 19K+ is . . .

a)

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

b)

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

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d1

d)

1s2 2s2 2p6 3s2 3p6

30.

A three-dimensional region around a nucleus where an electron may be found is called ---?

a)

orbital

b)

circuit

c)

circle

d)

orbit

31.

What is the electronic configuration for Phosphorus atom ? (15P)

a)

1s2 2s2 2p6 3s2

b)

1s2 2s2 2p6 3s2 3p5

c)

1s2 2s2 2p3

d)

1s2 2s2 2p6 3s2 3p3

32.

The trend seen in the periodic table for valence electron number is:

a)

they decrease across a period and match the group number.

b)

they increase across a period and match the group number.

c)

they decrease across a period and match the period number.

d)

they increase across a period and match the period number.

33.

As you move down the periodic table atoms get bigger. This is because ___________.

a)

The atoms have more protons.

b)

The atoms have more mass.

c)

The atoms have more energy levels

d)

The atoms have more nuetrons

34.

Electronegativity is...

a)

how easy it is to make friends.

b)

how good an atom is at attracting electrons

c)

the ability of an atom to lose electrons

d)

the energy required to remove an electron from a specific atom

35.

Which of the following elements has the smallest atomic radius?

a)

Aluminum (Al)

b)

Sodium (Na)

c)

Sulfur (S)

d)

Chlorine (Cl)

36.

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

a)

Germanium (Ge)

b)

Antimony (Sb)

c)

Neon (Ne)

d)

Carbon (C)

37.

The minimum energy required to remove an electron from the ground state of an atom

a)

energy levels

b)

electron configuration

c)

ionization energy

d)

ionic bond

38.

Our modern Periodic Table is organized by increasing....

a)

atomic number

b)

alphabetical order

c)

oxidation numbers

d)

average atomic mass

39.

What is the name of family I

a)

Alkali Metals

b)

Alkaline Earth Metals

c)

Boron Family

d)

Halogen Family

40.

Families all have similar

a)

Names

b)

atomic masses

c)

properties

d)

atomic numbers

41.

Which has a lower ionization energy: Lithium or Potassium?

a)

Lithium (Li)

b)

Potassium (K)

42.

An element that has the electron configuration [Ne]3s2 3p5 is in group

a)

17

b)

5

c)

7

d)

3

43.

In the periodic table diagram, the far-right vertical group is highlighted. These are the

a)

none of these

b)

noble gases

c)

alkaline earth metals

d)

halogens

e)

alkali metals

44.

In the periodic table diagram, the far-right vertical group is highlighted. These are the

a)

alkaline earth metals

b)

alkali metals

c)

halogens

d)

none of these

e)

noble gases

45.

In the periodic table diagram, a staircase-shaped band along the metal–nonmetal boundary is highlighted. These elements are

a)

nonmetals

b)

metals

c)

metalloids

46.

How does the atomic radius affect the reactivity of alkali metals?

a)

Smaller atomic radius increases reactivity

b)

Reactivity is determined by atomic mass

c)

Larger atomic radius increases reactivity

d)

Atomic radius has no effect on reactivity

47.

Which of the following generally applies to the noble gases?

a)

high ionization energy, low electronegativity, low reactivity

b)

high ionization energy, high electronegativity, high reactivity

c)

low ionization energy, low electronegativity, low reactivity

d)

high ionization energy, low electronegativity, high reactivity

48.

What elements have zero electronegativity?

a)

metals

b)

nonmetals

c)

noble gases

d)

metalloids

49.
In Dalton's Atomic Theory, all elements consist of __________ that cannot be divided.
a)
Atoms
b)
Parts
c)
Molecules
d)
Hydrogen
50.
Which of these particles was discovered first?
a)
Protons
b)
Electrons
c)
Neutrons
d)
Quarks
51.
While making his model of an atom, what structure did Rutherford discover (containing protons and neutrons)?
a)
the Nucleus
b)
the Electron Cloud
c)
the quarks
d)
the atomic mass
52.

Which of the following determines the identity of an element?

a)

number of protons

b)

atomic mass

c)

number of neutrons

d)

number of shells

53.

What does the 6 represent?

a)

Atomic mass

b)

atomic number

c)

chemical symbol

d)

element name

54.

Which of the following statements best describes the location of protons in an atom?

a)

Protons are located in the electron cloud.

b)

Protons are located in the nucleus.

c)

Protons are located between the electron cloud and the nucleus.

d)

Protons are located outside the atom.

55.

An aluminum isotope consists of 13 protons, 13 electrons, and 14 neutrons. What is its mass number?

a)

13

b)

27

c)

40

d)

14

56.

An aluminum isotope consists of 13 protons, 13 electrons, and 14 neutrons. What is its atomic number number?

a)

13

b)

27

c)

40

d)

14

57.

Atoms of the same element, with different numbers of neutrons are called what?

a)

Isomers

b)

Replications

c)

Isotopes

d)

Bonded Pairs

58.

dense center of an atom

a)

nucleus

b)

proton

c)

electron cloud

d)

electron region

59.

What is an alpha particle?

a)

It is a dominant particle in a subatomic world

b)

It is a high-energy particle that has 2+ charge

c)

It is a high-energy particle that has 2- charge

d)

It is a helium atom with a neutral charge

60.

Which of the following is the best evidence that the particles that make up a cathode ray had a negative charge?

a)

The particles were produced by many different metals.

b)

The ray was attracted toward a positive electric field.

c)

Line emission spectra for an element are always the same.

d)

The ray caused a phosphorescent screen to glow.

61.

Choose one of the conclusions that Ernest Rutherford made based on the experimental results of his Gold-Foil experiment

a)

He concluded that the atom is indivisible

b)

He concluded that the atom is mostly empty space

c)

He concluded that the atom has neutrons

d)

He concluded that the atom is tightly packed with subatomic particles all mixed together

62.
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
63.
5. What is it called when a solid turns directly into a gas?
a)
Sublimation
b)
Condensation
c)
Liquid
64.
Deposition is the opposite of sublimation.
a)
True
b)
False
65.
4. What type of state of matter is a gas that has electrons flowing through it?
a)
Gas
b)
Liquid
c)
Plasma
d)
Solid
66.
This state of matter has a definite volume but an indefinite shape and takes the shape of its container.
a)
Liquid 
b)
Solid 
c)
Gas
67.

The different substances in a mixture

a)

keep their physical properties

b)

form new molecules

c)

cannot be separated

d)

combine chemically

68.

Matter can be classified as either a __________ or a _____________.

a)

Element or a Compound

b)

Compound or a Solid

c)

Pure Substance or a Mixture

d)

Mixture or a Solid

69.

Which of the following is an example of a compound?

a)

Titanium

b)

Dry Ice

c)

Radium

d)

Helium

70.

Which of the following is a homogeneous mixture?

a)

Diamond

b)

Milk

c)

Sulfuric Acid

d)

Iron

71.

Elements and Compounds are classified as _______.

a)

Heterogeneous mixtures

b)

Homogeneous mixtures

c)

Pure substances

d)

Unpure substances

72.

Properties that DO depend on the amount of matter present.

a)

Mass

b)

Hardness

c)

Extensive

d)

Intensive

73.

Which of the following is an extensive property?

a)

Color

b)

Mass

c)

Odor

d)

Luster

74.

Which is an example of a chemical change?

a)

A chemical going form a liquid to a solid

b)

A chemical going from a solid to a gas

c)

Bending a piece of wire until it breaks

d)

The formation of bubbles when two chemicals are put together.

75.

Which mixture type can also be called a solution?

a)

Heterogeneous

b)

Homogeneous

c)

Elements

d)

Compounds

76.
When an unstable radioactive atom decays, it usually turns into:
a)
a more stable atom
b)
a less stable atom
c)
the exact same atom but with less pure energy
d)
empty space
77.

AZX* --> AZX + 00 γ\gamma  

a)

alpha decay

b)

beta positive decay

c)

beta negative decay

d)

electron capture

e)

gamma decay

78.

24094Pu —› ____ + 42He

a)

23692U

b)

24796Cm

c)

24493Np

d)

24295Am

79.
Solve this equation for alpha decay.
85209At = ___ + 24He
a)
83205Bi
b)
86209Rn
c)
81207Tl
d)
85208At
80.

Define nucleon number.

a)

Number of neutrons in an atomic nucleus

b)

Number of nucleons in an atomic nucleus

c)

Number of protons and neutrons around a nucleus

d)

Total number of protons and neutrons in an atomic nucleus

81.

Any reaction that involves the particles in the nucleus of an atom are called ________?

a)

Fission

b)

Nuclear Reaction

c)

Fusion

d)

Particle Accelerator

82.
What makes something radioactive?
a)
elements with an atomic number above 81
b)
an unstable nucleus
c)
contaminated sewage
d)
It decays over time
83.

13755Cs —› ____ + 0-1e

a)

17872Hf

b)

13753I

c)

14154Xe

d)

13756Ba

84.
Has the symbol
a)
Alpha
b)
Beta
c)
Gamma
85.
If X is the symbol for an element, which of the following two symbols represent    isotopes of the same element?     I. 7735X  II. 7733X  III. 8137X  IV. 8135 X
a)
I and II
b)
III and IV
c)
I and IV
d)
I and III
86.
Has the symbol
a)
Alpha
b)
Beta
c)
Gamma
87.
Has the symbol
a)
Alpha
b)
Beta 
c)
Gamma
88.

AZX --> AZ-1Y + 0+1e

a)

alpha decay

b)

beta positive decay

c)

beta negative decay

d)

electron capture

e)

gamma decay

89.

In a correctly written symbol what would be located in the "Z" position?

a)

number of neutrons

b)

atomic number

c)

number of electrons

d)

mass number

90.
Has a mass of 0 and a charge of 0
a)
Alpha
b)
Beta
c)
Gamma
91.

An alpha particle consists of...

a)

2 protons and 2 neutrons

b)

1 proton and 1 neutron

c)

2 protons and 1 neutron

d)

1 proton and 2 neutrons

92.
Has a mass of 1/1837 and a charge of -1
a)
Alpha
b)
Beta
c)
Gamma
93.
The electron configuration of an atom is 1s22s22p6.  The number of valence electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
94.

Below are the correct answer of the writing of electron configuration, except... .

a)

6f2

b)

2p5

c)

3d7

d)

4s3

95.

which of the following is the correct distribution of the last sub level in oxygen (O8) ?

a)

a

b)

b

c)

c

d)

d

96.

Write the electron configuration

a)

1s22s22p6

b)

1s12s12p3

c)

1s22s22p63s2

d)

1s22s22p63s3

97.

The electron configuration for Nitrogen is 1s22s22p3. What would the electron configuration of the ion look like if Nitrogen has a -3 charge?

a)

1s22s22p6

b)

1s22s2

c)

1s22s22p3

d)

1s22s22p5

98.

The only noble gas that does not end with ns2, np6 is ………..

a)

Radon

b)

argon

c)

neon

d)

helium

99.

The actual electronic configuration of chromium

(a)  

100.

Look at the periodic table to answer the questions

(a)  

Similar Resources on Wayground

3.10 | Elements You Must Know

102 questions

3.10 | Elements You Must Know

quiz

Worksheet

•

10th - 12th Grade

Chemistry Final Review

103 questions

Chemistry Final Review

quiz

Worksheet

•

9th Grade

Chemistry Review Quiz Ch1-Ch2a

100 questions

Chemistry Review Quiz Ch1-Ch2a

quiz

Worksheet

•

9th Grade - University

Chemistry Review Packet 2nd 9Wks 2025

105 questions

Chemistry Review Packet 2nd 9Wks 2025

quiz

Worksheet

•

10th Grade

CH06A Nomenclature - Types of Compounds

98 questions

CH06A Nomenclature - Types of Compounds

quiz

Worksheet

•

10th - 11th Grade

NGSS Chemistry Unit 4 Review

97 questions

NGSS Chemistry Unit 4 Review

quiz

Worksheet

•

10th Grade

Chemistry 11 Semester 2 Review

100 questions

Chemistry 11 Semester 2 Review

quiz

Worksheet

•

11th Grade