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Fall Final Review - Classification of Matter

Total questions: 114

Worksheet time: 1hrs 6mins

Name
Class
Date
1.

Who discovered the nucleus was positive and dense?

a)

Rutherford

b)

Thomson

c)

Bohr

d)

Dalton

2.

What experiment was used to discover the electron?

a)

Cathode Ray

b)

Gold Foil

c)

Oil Drop

d)

Photoelectric

3.

Who discovered the electron?

a)

Thomson

b)

Rutherford

c)

Bohr

d)

Newton

4.

What experiment was used to discover the proton?

a)

Gold foil

b)

Oil drop

c)

Cathode ray

d)

Photoelectric

5.

Who included energy levels in his model?

a)

Bohr

b)

Dalton

c)

Thomson

d)

Rutherford

6.

What particle(s) are found inside the nucleus?

a)

Protons

b)

Electrons

c)

Neutrons

d)

Photons

7.

What particle(s) are found outside the nucleus?

a)

Electrons

b)

Protons

c)

Neutrons

d)

Quarks

8.

Atoms and ions are different because:

a)

Atoms have equal numbers of protons and electrons, while ions have unequal numbers.

b)

Atoms and ions both have a net charge.

c)

Atoms are always larger than ions.

d)

Atoms and ions have the same number of neutrons.

9.

The mass of which subatomic particle is negligible (too small to matter)?

a)

Electron

b)

Proton

c)

Neutron

d)

Alpha particle

10.

What part of an atom carries most of its mass?

a)

Nucleus

b)

Electron

c)

Proton

d)

Neutron

11.

Rubidium is a soft, silvery-white metal that has two common isotopes, 85Rb and 87Rb. If the abundance of 85Rb is 72.2% and the abundance of 87Rb is 27.8%, what is the average atomic mass of rubidium? SHOW ALL WORK (mass)(%) + (mass)(%) + (mass)(%) + ... = average atomic mass

a)

Average atomic mass = (85 × 0.722) + (87 × 0.278) = 85.56 amu

b)

Average atomic mass = (85 × 0.278) + (87 × 0.722) = 86.56 amu

c)

Average atomic mass = (85 × 0.500) + (87 × 0.500) = 86.00 amu

d)

Average atomic mass = (85 × 0.600) + (87 × 0.400) = 85.80 amu

12.

Which scientists are responsible for creating/organizing the periodic table and why did each scientist organize the periodic table as they did?

a)

Mendeleev organized the periodic table by increasing atomic mass and grouped elements with similar properties together.

b)

Dalton organized the periodic table by arranging elements alphabetically.

c)

Thomson organized the periodic table by increasing atomic number only.

d)

Rutherford organized the periodic table by grouping elements based on their color.

13.

Which scientists are responsible for creating/organizing the periodic table and why did each scientist organize the periodic table as they did?

a)

Moseley organized the periodic table by increasing atomic number.

b)

Mendeleev organized the periodic table by increasing atomic mass.

c)

Dalton organized the periodic table by atomic weight.

d)

Thomson organized the periodic table by electron configuration.

14.

Label the following increasing trends on the periodic table: ionization energy, electronegativity, and atomic radius.

a)

Ionization energy and electronegativity increase across a period; atomic radius increases down a group.

b)

Atomic radius and ionization energy increase across a period; electronegativity increases down a group.

c)

Electronegativity and atomic radius increase across a period; ionization energy increases down a group.

d)

Ionization energy, electronegativity, and atomic radius all increase down a group.

15.

Which element has the lowest electronegativity?

a)

Sulfur

b)

Calcium

c)

Chlorine

d)

Strontium

16.

Which element has the largest atomic radius?

a)

Sulfur

b)

Calcium

c)

Chlorine

d)

Strontium

17.

Which element has the highest ionization energy?

a)

Sulfur

b)

Calcium

c)

Chlorine

d)

Strontium

18.

Which element is least likely to form a positive ion?

a)

Sulfur

b)

Calcium

c)

Chlorine

d)

Strontium

19.

Which element is most likely to form a positive ion?

a)

Sulfur

b)

Calcium

c)

Chlorine

d)

Strontium

20.

Which element has the largest ionic radius?

a)

Sulfur

b)

Calcium

c)

Chlorine

d)

Strontium

21.

Which of the atoms has the highest Ionization energy? _____ Why?

a)

C. It has the fewest electron shells, so electrons are held more tightly.

b)

A. It has the most electron shells, so electrons are held loosely.

c)

B. It has the largest atomic radius, so electrons are farther from the nucleus.

d)

D. It has the most protons, so electrons are easily lost.

22.

Which of the atoms has the smallest radius? _____ Why?

a)

C. Fewer electron shells mean a smaller radius.

b)

A. More electron shells mean a smaller radius.

c)

B. More protons mean a larger radius.

d)

D. Fewer protons mean a larger radius.

23.

Write electron configurations for Magnesium

a)

1s2 2s2 2p6 3s2

b)

1s2 2s2 2p6 3p2

c)

1s2 2s2 2p4 3s2

d)

1s2 2s2 2p6 4s2

24.

Write electron configurations for Selenium

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4

b)

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

c)

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

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d6 4p4

25.

Write electron configurations for Gallium

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1

b)

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

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d5 4p1

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

26.

Write electron configurations for Krypton

a)

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

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3

27.

Write electron configurations for Potassium

a)

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

b)

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

c)

1s2 2s2 2p6 3s2 3p5 4s2

d)

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

28.

Write electron configurations for Oxygen

a)

1s2 2s2 2p4

b)

1s2 2s2 2p6

c)

1s2 2s2 2p2

d)

1s2 2s2 2p5

29.

Write electron configurations for Iodine

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p5

b)

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

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p4

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p3

30.

What is the number of valence electrons for Group 1A?

a)

1

b)

2

c)

4

d)

8

31.

What is the charge for Group 1A?

a)

+1

b)

-1

c)

+2

d)

0

32.

Complete the following table: Give an example of a Lewis Dot structure for Group 1A.

a)

• (for Na or Li, a single dot)

b)

•• (for Na or Li, two dots)

c)

No dots (for Na or Li)

d)

• (for Na or Li, three dots)

33.

What is the number of valence electrons for Group 2A?

a)

2

b)

1

c)

3

d)

4

34.

What is the charge for Group 2A?

a)

+2

b)

+1

c)

-2

d)

0

35.

Complete the following table: Give an example of a Lewis Dot structure for Group 2A.

a)

•• (for Mg or Ca, two dots)

b)

• (for Mg or Ca, one dot)

c)

••• (for Mg or Ca, three dots)

d)

No dots (for Mg or Ca)

36.

What is the number of valence electrons for Group 3A?

a)

3

b)

1

c)

2

d)

4

37.

What is the charge for Group 3A?

a)

+3

b)

-1

c)

+1

d)

-3

38.

Complete the following table: Give an example of a Lewis Dot structure for Group 3A.

a)

••• (for Al, three dots)

b)

•••• (for Al, four dots)

c)

•• (for Al, two dots)

d)

• (for Al, one dot)

39.

What is the number of valence electrons for Group 4A?

a)

4

b)

2

c)

6

d)

8

40.

What is the charge for Group 4A?

a)

±4 or none (varies)

b)

+2

c)

-1

d)

+1

41.

Complete the following table: Give an example of a Lewis Dot structure for Group 4A.

a)

•••• (for C or Si, four dots)

b)

••• (for N or P, three dots)

c)

•• (for O or S, two dots)

d)

• (for H, one dot)

42.

What is the number of valence electrons for Group 5A?

a)

5

b)

3

c)

6

d)

7

43.

What is the charge for Group 5A?

a)

-3

b)

+1

c)

-1

d)

+3

44.

Complete the following table: Give an example of a Lewis Dot structure for Group 5A.

a)

••••• (for N or P, five dots)

b)

•••• (for N or P, four dots)

c)

••• (for N or P, three dots)

d)

•••••• (for N or P, six dots)

45.

What is the number of valence electrons for Group 6A?

a)

6

b)

4

c)

5

d)

7

46.

What is the charge for Group 6A?

a)

-2

b)

+2

c)

-1

d)

+1

47.

Complete the following table: Give an example of a Lewis Dot structure for Group 6A.

a)

•••••• (for O or S, six dots)

b)

••••• (for O or S, five dots)

c)

••••••• (for O or S, seven dots)

d)

•••• (for O or S, four dots)

48.

What is the number of valence electrons for Group 7A?

a)

7

b)

5

c)

3

d)

8

49.

What is the charge for Group 7A?

a)

-1

b)

+1

c)

0

d)

-2

50.

Complete the following table: Give an example of a Lewis Dot structure for Group 7A.

a)

••••••• (for F or Cl, seven dots)

b)

••••• (for F or Cl, five dots)

c)

•••••• (for F or Cl, six dots)

d)

•••••••• (for F or Cl, eight dots)

51.

What is the number of valence electrons for Group 8A?

a)

8

b)

6

c)

4

d)

2

52.

What is the charge for Group 8A?

a)

0

b)

+1

c)

-1

d)

+2

53.

Complete the following table: Give an example of a Lewis Dot structure for Group 8A.

a)

•••••••• (for Ne or Ar, eight dots)

b)

•••• (for Be, four dots)

c)

•••••• (for O, six dots)

d)

••• (for Li, three dots)

54.

Label the electromagnetic spectrum diagram with the following: Where is low energy?

a)

On the right, near radio waves

b)

On the left, near gamma rays

c)

In the middle, near visible light

d)

On the left, near ultraviolet waves

55.

Label the electromagnetic spectrum diagram with the following: Where is high energy?

a)

On the left, near gamma rays

b)

On the right, near radio waves

c)

In the middle, near visible light

d)

On the right, near infrared

56.

Label the electromagnetic spectrum diagram with the following: Where is low frequency?

a)

On the right, near radio waves

b)

On the left, near gamma rays

c)

In the middle, near visible light

d)

On the left, near ultraviolet waves

57.

Label the electromagnetic spectrum diagram with the following: Where is high frequency?

a)

On the left, near gamma rays

b)

On the right, near radio waves

c)

In the middle, near visible light

d)

On the right, near infrared

58.

Label the electromagnetic spectrum diagram with the following: Where is low wavelength?

a)

On the left, near gamma rays

b)

On the right, near radio waves

c)

In the middle, near visible light

d)

On the right, near infrared

59.

Label the electromagnetic spectrum diagram with the following: Where is high wavelength?

a)

On the right, near radio waves

b)

On the left, near gamma rays

c)

In the middle, near visible light

d)

On the left, near ultraviolet rays

60.

Arrange the following types of electromagnetic radiation in order of increasing wavelength: Gamma rays, X-rays, Ultraviolet, Visible light.

a)

Gamma rays, X-rays, Ultraviolet, Visible light

b)

Visible light, Ultraviolet, X-rays, Gamma rays

c)

Ultraviolet, Visible light, X-rays, Gamma rays

d)

Gamma rays, Ultraviolet, X-rays, Visible light

61.

Name or write the following compounds. a. CaCl₂ ____________

a)

Calcium chloride

b)

Calcium chlorate

c)

Calcium carbonate

d)

Calcium chlorite

62.

Name or write the following compounds.
b. Potassium bromide ____________

a)

KBr

b)

KBrO3

c)

K2Br

d)

K2BrO3

63.

Name or write the following compounds. c. K₂S

a)

Potassium sulfide

b)

Potassium sulfate

c)

Potassium sulfite

d)

Potassium nitrate

64.

Name or write the following compounds.
d. NaHCO₃

a)

Sodium bicarbonate (or Sodium hydrogen carbonate)

b)

Sodium carbonate

c)

Sodium hydroxide

d)

Sodium chloride

65.

Name or write the following compounds. e. H₂O ____________

a)

Water

b)

Hydrogen peroxide

c)

Hydrogen oxide

d)

Hydroxide

66.

Name or write the following compounds. f. Iron (III) oxide ____________

a)

Fe₂O₃

b)

FeO

c)

Fe₃O₄

d)

Fe₂O

67.

Name or write the following compounds. g. Cl₂ ____________

a)

Chlorine

b)

Chloride

c)

Chlorate

d)

Chloroform

68.

Name or write the following compounds. h. NH₃ ____________

a)

Ammonia

b)

Nitrogen trioxide

c)

Ammonium nitrate

d)

Nitrous oxide

69.

Name or write the following compounds. i. SCl₂ ____________

a)

Sulfur dichloride

b)

Sulfur chloride

c)

Sulfur monochloride

d)

Sulfur trichloride

70.

Name or write the following compounds. j. Al₂O₃ ____________

a)

Aluminum oxide

b)

Aluminum hydroxide

c)

Aluminum carbonate

d)

Aluminum sulfate

71.

Name or write the following compounds. k. Carbon tetrachloride ____________

a)

CCl₄

b)

COCl₂

c)

CCl₃

d)

C₂Cl₄

72.

Name or write the following compounds. l. Calcium carbonate ____________

a)

CaCO₃

b)

CaSO₄

c)

CaCl₂

d)

CaO

73.

What is the correct Lewis electron-dot structure for the compound formed between magnesium and fluorine?

a)

Mg :F:

b)

Mg[+2][F:-]

c)

[Mg2+][F:-][F:-]

d)

:F:Mg:F:

74.

Which of the following choices shows the correct Lewis electron-dot diagram for a molecule of chlorine, Cl₂?

a)

[Cl:Cl]

b)

[:Cl:Cl:]

c)

[:Cl::Cl:]

d)

[:Cl:Cl:]

75.

Which pair of elements would most likely bond to form a covalently bonded compound?

a)

sodium and fluorine

b)

barium and chlorine

c)

phosphorus and oxygen

d)

magnesium and sulfur

76.

Why can metals be hammered into sheets and drawn into wire?

a)

Mobile valence electrons involved in metallic bonding can be pushed or pulled past each other.

b)

Delocalized inner electrons involved in metallic bonding can be pushed or pulled past each other.

c)

Shared inner electrons involved in metallic bonding can be pushed or pulled past each other.

d)

Transferred valence electrons involved in metallic bonding can be pushed or pulled past each other.

77.

Ionic bonds are bonds between atoms in which one atom donates electrons to another atom in order to become stable. In this bond, the resulting atoms become oppositely charged and attracted to each other. Which of the following atoms would combine to form an ionic bond?

a)

K and Cl

b)

C and H

c)

O and P

d)

O and H

78.

Identify the type of bond formed between the following pairs of elements: a) Ca and Cl b) S and O c) Cu and Zn

a)

a) Ionic, b) Covalent, c) Metallic

b)

a) Covalent, b) Ionic, c) Metallic

c)

a) Metallic, b) Covalent, c) Ionic

d)

a) Covalent, b) Metallic, c) Ionic

79.

Identify which of the following compounds is ionic and which is covalent.

a)

NaCl is ionic, H2O is covalent

b)

NaCl is covalent, H2O is ionic

c)

Both NaCl and H2O are ionic

d)

Both NaCl and H2O are covalent

80.

Which of the following best describes the process involved in forming an ionic compound between two elements?

a)

Transfer of valence electrons from one atom to another resulting in the formation of ions.

b)

Sharing of valence electrons between atoms to achieve stability.

c)

No change in the valence electrons of the atoms involved.

d)

Formation of a metallic bond by pooling electrons among atoms.

81.

Which of the following are metals? Put a star by the metals that can have multiple charges (transition metals).

a)

barium

b)

calcium

c)

chromium

d)

lead

e)

gold

82.

The Electron sea model proposes that metal atoms:

a)

share a sea of delocalized electrons.

b)

form ionic bonds with each other.

c)

have tightly bound electrons.

d)

do not conduct electricity.

83.

Delocalized electrons are:

a)

electrons that are not associated with a single atom or bond and can move freely within a structure

b)

electrons that are tightly bound to a single atom

c)

electrons that only exist in ionic compounds

d)

electrons that are found only in noble gases

84.

Metals are good conductors of electricity and heat because:

a)

they have free electrons that move easily.

b)

they are soft and malleable.

c)

they have high melting points.

d)

they are shiny and lustrous.

85.

Metals are malleable and ductile because:

a)

their atoms are arranged in layers that can slide over each other.

b)

they have a high melting point.

c)

they are good conductors of electricity.

d)

they react easily with acids.

86.

Which of the following electron dot formulas for chloromethane (CH₃Cl) satisfy the octet rule?

a)

[diagram a]

b)

[diagram b]

c)

[diagram c]

d)

[diagram d]

87.
Which wave has the largest wavelength?
a)
A
b)
B
c)
C
d)
None (same wavelength)
88.

Which color has the longest wavelength?

a)

Yellow

b)

Red

c)

Green

d)

Purple

89.
Which type of light has the highest energy of this group?
a)
red
b)
yellow
c)
green
d)
blue
90.
Which type of light has the lowest energy of this group?
a)
Radio
b)
Microwave
c)
Infrared
d)
Ultraviolet
91.
This color in the visible part of the spectrum has the lowest energy. 
a)
Blue
b)
Green
c)
Red
d)
Violet
92.

What is the atomic number of oxygen?

a)

5

b)

Sandwich

c)

8

d)

17

93.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
94.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
95.
a)
Periods
b)
Groups
96.
What is an ion?
a)
A Charged Atom
b)
A Large Atom
c)
A Small Atom
d)
A Cute Atom
97.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
98.
Most of the elements on the periodic table are classified as _____.
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Periods
99.
What is an isotope? 
a)
A charged atom
b)
An atom with different amounts of neutrons
c)
An atom with different amounts of protons
d)
A neutral atom
100.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
101.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
102.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
103.
How many electrons can the s sublevel hold?
a)
14
b)
10
c)
2
d)
6
104.

How many electrons does sulfur have

a)

16

b)

32

c)

48

d)

12

105.
What is the atomic number of this atom?
a)
4
b)
5
c)
9
d)
none of the above
106.
Beryllium is in group number______.
a)
Group 2
b)
Group 3
c)
Group 4
d)
Group 7
107.

How many protons are in Gold

a)

79

b)

197

c)

118

d)

276

108.
Atoms are made up of three basic parts, which are -
a)
Protons, neutrons, electrons
b)
neutrinos, protons, neutrons
c)
quarks, protons, electrons
d)
electrons, neutrons, and quarks
109.
What is the atomic number of this atom?
a)
7
b)
14
c)
21
d)
none of the above
110.

How many neutrons does Sodium (Na) have?

a)

11

b)

23

c)

12

d)

22.98977

111.

Which two elements have properties in common?

a)

Nitrogen and Phosphorous

b)

Oxygen and Nitrogen

c)

Sulfur and Nitrogen

112.

What group is highlighted here on the periodic table (Group 2A)?

a)

Noble Gases

b)

Halogens

c)

Alkali Metals

d)

Alkaline Earth Metals

113.
Which elements have the most similar chemical properties?
a)
K and Na
b)
K and Ca
c)
K and Cl
d)
K and S
114.

Which is true about the following chlorine atom?

a)

17 protons and 36 neutrons

b)

17 protons and 19 electrons

c)

17 protons and 19 neutrons

d)

36 protons and 17 neutrons

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