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Worksheets

8th Comp #1

Total questions: 91

Worksheet time: 56mins

Name
Class
Date
1.

If you completely dissolve NaCl in pure, distilled water, the result would be classified as:

a)

Element

b)

Homogenous mixture

c)

Compound

d)

Heterogenous mixture

2.

Which is an example of a heterogeneous mixture?

a)

Oil and water

b)

Calcium carbonate

c)

Sodium metal

d)

Air

3.

A pure substance made up of only one type of atom is called a(n) (a)   .

4.

Which of the following is an element?

a)

HCO₃

b)

KCl

c)

CO

d)

Cl₂

5.

Which of the following is a compound?

a)

Crude oil

b)

Water

c)

Steel

d)

Neon

6.

Combustion reactions always form carbon dioxide and water as products. Carbon dioxide is a:

a)

Pure element

b)

Ionic compound

c)

Covalent compound

d)

Mixture of elements

7.

5 ml of ethanol is added to 200 ml of water. In this mixture, ethanol is called:

a)

Solute

b)

Element

c)

Solvent

d)

Suspension

8.

Which of these common substances is a homogeneous mixture?

a)

Table salt

b)

Sand and water

c)

Salt water

d)

Pure water

9.

What would be the best method for separating tea leaves from a pot of tea?

a)

Distillation

b)

Chromatography

c)

Filtration

d)

Decanting

10.

Liquid Isopropyl Alcohol (boiling point of 82.6 °C) and liquid water (boiling point of 100 °C) are mixed together to form a homogenous mixture. What is the best technique for separating this mixture?

a)

Chromatography

b)

Filtration

c)

Distillation

d)

Decantation

11.

A method to physically separate a mixture using a mobile and a stationary phase, is called (a)   .

12.

Distillation is a separation method that takes advantage of the difference in (a)   of the components in the mixture.

13.

Barium sulfate is not soluble in water. Which separation technique would work best to remove it from the water?

a)

Decantation

b)

Chromatography

c)

Centrifugation

d)

Filtration

14.

Salt can be separated from saltwater solution by:

a)

Filtration

b)

Distillation

c)

Evaporation

d)

Salt cannot be separated from saltwater solution.

15.

Which of the following is an example of a chemical property?

a)

Shiny

b)

Brittle

c)

Malleable

d)

Reactive with water

16.

Which observation is a sign of a chemical change?

a)

A rotting potato gives off a bad smell.

b)

A melting block of ice leaves a puddle.

c)

Crumbling of cookies.

d)

Iron pellets melting at 1500°C

17.

Which of the following is a chemical change?

a)

Burning

b)

Dissolving

c)

Boiling

d)

Sublimating

18.

An example of a physical change is:

a)

A reaction of sodium with water.

b)

Burning wood.

c)

Breaking a glass.

d)

Baking a cake.

19.

All of the following are properties of SO₂. Which one is a physical property?

a)

It reacts with oxygen to form SO₃²⁻.

b)

It forms acid rain in the atmosphere.

c)

It condenses to a liquid at 14°F.

d)

It is a by-product of burning coal.

20.

Which of the following properties would NOT help you to identify an unknown substance?

a)

Mass

b)

Density

c)

Color

d)

Solubility

21.

Which of the following is a physical property?

a)

Density is 0.534 g/cm³

b)

Produces LiOH and H₂ in water

c)

Reactive with acid.

d)

Rusts in the presence of air.

22.

Which sample of matter has particles with fast movement and random motion?

a)

He (g)

b)

H₂O (s)

c)

H₂O (l)

d)

He (s)

23.

In which phase does a substance have a definite volume but no definite shape?

a)

Liquid

b)

Gas

c)

Solid

d)

Plasma

24.

If a substance has fast moving particles that rapidly bounce off one another, it is currently in a:

a)

Solid state

b)

Gaseous state

c)

Liquid state

d)

Plasma state

25.

If water droplets form from the vapor in the air on the outside of my cold-water bottle, what process is taking place?

a)

Evaporation

b)

Melting

c)

Condensation

d)

Freezing

26.

Which of the following diagrams have definite volume?

a)

A

b)

C

c)

B

d)

A and C

27.

A measure of the average KE of particles is the (a)   .

28.

Radiation involves the transfer of heat via:

4 lines
29.

Cindy heated a pot of hot water to make ramen by transferring 1800 calories of energy to the water using a stove top. If the water is the system, is this process endothermic or exothermic? Explain.

a)

Exothermic, because water absorbed heat from the stove top, raising its temperature.

b)

Exothermic, because the stove top absorbed heat released by the water.

c)

Endothermic, because water absorbed heat from the stove top, raising its temperature.

30.

When sweat evaporates from the skin, it cools the body down. Which of the following statements is true about this process?

a)

Sweat evaporating is exothermic. Sweat absorbs heat from the skin in order to evaporate.

b)

Sweat evaporating is endothermic. Sweat absorbs heat from the skin in order to evaporate.

31.

Which heating method works well with solids and involves a substance transferring heat to another substance that it is in contact with?

a)

Convection

b)

Enthalpy

c)

Conduction

d)

Radiation

32.

Near the ceiling of a room the air is warmer. The warm air rises because of:

a)

Convection

b)

Enthalpy

c)

Conduction

d)

Radiation

33.

Which element below would form the charge of -3 when ionized?

a)

Boron

b)

Silicon

c)

Scandium

d)

Nitrogen

34.

Mr. Wade is reacting bromine with aluminum, creating a bright orange flame. During the reaction the bromine becomes an ion. What is the charge on bromine?

a)

Br⁺

b)

Br²⁺

c)

Br⁻

d)

Br₂⁻

35.

An atom of Ar contains 18 electrons. How many energy levels are needed to contain these electrons?

a)

1

b)

2

c)

3

d)

4

36.

What is the number of electrons in an Al³⁺ ion?

a)

3

b)

13

c)

10

d)

16

37.

Which element has three electron shells and five valence electrons?

a)

V

b)

Pd

c)

N

d)

Na

38.

Atoms to the left of the “staircase” on the periodic table that are shiny, conduct electricity and are malleable are:

a)

Metal and gain electrons, becoming negative.

b)

Metal and lose electrons, becoming positive.

c)

Nonmetal and gain electrons, becoming negative.

d)

Nonmetal and lose electrons, becoming negative.

39.

Which of the following elements is likely to be brittle as a solid and an insulator?

a)

Lithium

b)

Boron

c)

Titanium

d)

Phosphorus

40.

Which of the following is a property of non-metals?

a)

Dull

b)

Lustrous (shiny)

41.

The elements in Group 2 have similar chemical properties because each atom of these elements has the same:

a)

Atomic number

b)

Number of electron shells

c)

Mass number

d)

Number of valence electrons

42.

The most nonreactive (stable) group on the periodic table is

a)

Alkali metals

b)

Alkaline-earth metals

c)

Noble gases

d)

Halogens

43.

The most reactive elements on the periodic table are nonmetals and appear at room temperature as solid, liquids, and gases. To which family do they belong?

a)

Alkali metals

b)

Halogens

c)

Noble gases

d)

Transition metals

44.

Which element would you expect to have similar properties to oxygen?

a)

As

b)

Se

c)

Si

d)

Ne

45.

Put the following elements in order of increasing (smallest to largest) atomic radii: Ne, Fr, S, As, Ba

a)

S, As, Ba, Fr, Ne

b)

Ne, S, As, Ba, Fr

c)

Fr, Ba, As, S, Ne

d)

Ne, Fr, S, As, Ba

46.

The ionic radius of bromide is ____ than neutral bromine because ____.

a)

Smaller; an e- has been lost.

b)

Smaller; an e- has been gained.

c)

Larger; an electron has been lost.

d)

Larger; an electron has been gained.

47.

Put the following in order of increasing (smallest to largest) ionization energy: Ne, Fr, S, As, Ba

a)

S, As, Ba, Fr, Ne

b)

Ne, S, As, Ba, Fr

c)

Fr, Ba, As, S, Ne

d)

Ne, Fr, S, As, Ba

48.

Select the element with the lowest ionization energy. As, P, N, Sb

a)

N

b)

As

c)

P

d)

Sb

49.

Arrange the following elements by increasing Atomic Radius (left to right): N, K, Ga, Cs, Ne

a)

Cs, K, Ga, N, Ne

b)

Ne, N, Ga, K, Cs

c)

N, Ga, Ne, Cs, K

d)

Ga, N, Ne, K, Cs

50.

Which of the following properties increases as you move across a period from left to right? I. Electronegativity II. Ionization energy III. atomic radius

a)

I and II only

b)

II and III only

c)

I and III only

d)

I, II, and III

51.

Which of the following has the smallest ionic radius?

a)

O²⁻

b)

Na⁺

c)

F⁻

d)

Mg²⁺

52.

The atomic radius of helium is smaller than the atomic radius of hydrogen because:

a)

Hydrogen has less electrons, which makes the valence shell bigger.

b)

Helium has less protons, which makes it smaller.

c)

Hydrogen has more neutrons, so it has more mass.

d)

Helium has more protons that pull harder on the electron shells.

53.

Arrange the following elements by increasing Atomic Radius (left to right): N, K, Ga, Cs, Ne

a)

Cs, K, Ga, N, Ne

b)

Ne, N, Ga, K, Cs

c)

N, Ga, Ne, Cs, K

d)

Ga, N, Ne, K, Cs

54.

The atomic radius of helium is smaller than the atomic radius of hydrogen because:

a)

Hydrogen has less electrons, which makes the valence shell bigger.

b)

Helium has less protons, which makes it smaller.

c)

Hydrogen has more neutrons, so it has more mass.

d)

Helium has more protons that pull harder on the electron shells.

55.

Of the four elements Na, S, F and Cl, the MOST electronegative is

a)

Na

b)

F

c)

S

d)

Cl

56.

Which of the following has the highest electronegativity?

a)

Nitrogen

b)

Fluorine

c)

Bromine

d)

Arsenic

57.

Which of the following reasons best explains why Noble Gases are not electronegative?

4 lines
58.

Arrange the following elements in order of increasing Electronegativity: S, Li, Zn, Xe, Cl

a)

Xe < Li < Zn < S < Cl

b)

Cl < Xe < Zn < Li < S

c)

Li < Zn < S < Cl < Xe

d)

Zn < Li < S < Cl < Xe

59.

Choose the correct ranking for elements increasing (from lowest to highest) in electronegativity.

a)

K < O < Br < I

b)

He < F < Se < Sn

c)

Ag < Pt < Zr < Fr

d)

Na < Mg < C < F

60.

Put the following in order of increasing (smallest to largest) electronegativity: Ne, Fr, S, As, and Ba based on periodic trends:

a)

S, As, Ba, Fr, Ne

b)

Fr, Ba, As, S, Ne

c)

Ne, S, As, Ba, Fr

d)

Ne, Fr, Ba, As, S

61.

Which of the following elements has the lowest electronegativity?

a)

Iodine

b)

Chlorine

c)

Bromine

d)

Fluorine

62.

Which element would you expect to have similar properties to oxygen?

a)

As

b)

Se

c)

Si

d)

Ne

63.

Which combination of elements is most likely to produce a compound with ionic bonds?

a)

S and Br

b)

N and Cl

c)

Ni and Co

d)

V and Se

64.

An ionic bond forms between:

a)

Two nonmetals

b)

Two metalloids

c)

Two metals

d)

A metal and a nonmetal

65.

In the compound lead sulfide, PbS2, what charge would the lead ion have?

a)

-4

b)

+4

c)

-2

d)

+2

66.

What occurs when potassium reacts with chlorine to form potassium chloride?

a)

Electrons are shared and the bonding is ionic.

b)

Electrons are shared and the bonding is covalent.

c)

Electrons are transferred and the bonding is ionic.

67.

When a nonmetal forms an ionic bond, the nonmetal tends to do which of the following?

a)

Lose protons

b)

Gain electrons

c)

Lose electrons.

68.

What molecule would you predict Ca (calcium) and Cl (chlorine) form?

a)

CaCl

b)

Ca2Cl

c)

CaCl2

69.

If a molecule has a formula of AlX3, which of the following elements would be a reasonable ion for X?

(a)  

70.

Mystery element X reacts with oxygen and forms an ionic compound with the formula X2O. Which of the following families could we find element X in?

a)

Alkali metals

b)

Boron family

c)

Alkaline Earth metals

d)

Halogens

71.

What is the correct name for the compound ZnCl2?

a)

Zinc chloride

b)

Zinc (III) chloride

c)

Zinc chloride (II)

d)

Zinc dichloride

72.

What is the name of the following compound: Cr(C2H3O2)4 ?

a)

Chromium carbon oxide

b)

Chromium (IV) acetate

c)

Chromium (I) acetate

d)

Chromium acetate

73.

The charge on the indium ion in indium nitrate, In(NO3)3, is:

a)

+1

b)

+2

c)

+3

d)

+4

74.

What is the formula of the compound Iron (II) Phosphide?

a)

Fe₃PO₄

b)

Fe₂P₃

c)

Fe₃PO₃

d)

Fe₃P₂

75.

What is the formula for carbon tetrafluoride?

a)

C₄F

b)

C₄Fl

c)

CF₄

d)

CF₄I

76.

What is the name of this compound, Br₂O₇?

a)

Perbromate ion

b)

Oxygen bromide

c)

Dibromine heptoxygen

d)

Dibromine heptoxide

77.

Which of these compounds would NOT have covalent bonds?

a)

PCl₃

b)

C₂H₆

c)

K₂O

d)

H₂O₂

78.

The correct name for the compound N₂O₃ is

a)

Dinitrogen Trioxide

b)

Nitrogen (III) Oxide

c)

Nitrogen Oxide

d)

Nitrogen (II) Oxide

79.

Which of these pairs of elements can be joined by a covalent bond?

a)

C and K

b)

C and Fr

c)

C and Fe

d)

C and Cl

80.

Which of the following is the correct formula for hexanitrogen tetrabromide?

a)

N₄Br₄

b)

N₅Br₆

c)

N₆Br₄

d)

N₈Br₃

81.

In covalent bonding, electrons are ________ whereas in ionic bonding, electrons are ________

4 lines
82.

Acetylene is C₂H₂. What sort of bond joins the two carbons in the Lewis dot structure?

4 lines
83.

When diatomic oxygen (O₂) is formed, we find that it is symmetrical. Which of the following best describes the Lewis structure for each oxygen?

a)

1 bonding pair, 3 lone pairs

b)

2 bonding pairs, 2 lone pairs

c)

3 bonding pairs, 1 lone pair

d)

4 bonding pairs, 0 lone pairs

84.

In the Lewis structure of a water molecule (H₂O) how many bonding pairs and lone pairs are on the oxygen atom?

a)

3 bonding pairs, 1 lone pair

b)

1 bonding pair, 3 lone pairs

c)

2 bonding pairs, 0 lone pairs

d)

2 bonding pairs, 2 lone pairs

85.

The Lewis Dot Structure of NH₃ contains:

a)

Three single bonds and no lone pairs of electrons.

b)

Three single bonds and one lone pair of electrons.

c)

Two single bonds and two lone pair of electrons.

d)

Two single bonds and three lone pairs of electrons.

86.

If a central atom is bonded to three atoms and has no lone pairs, what is the molecular geometry of the molecule?

a)

Trigonal Planar

b)

Trigonal bipyramidal

c)

Tetrahedral

d)

Linear

87.

What are the bond angles for a molecule with tetrahedral geometry?

a)

90°

b)

120°

c)

180°

d)

109°

88.

What is the geometry of NH₃?

a)

Bent

b)

Trigonal Pyramidal

c)

Trigonal Planar

d)

Tetrahedral

89.

What geometry does ozone (O₃) have?

a)

Trigonal Planer

b)

Trigonal Planar

c)

Bent (109°)

d)

Linear

90.

What is the molecular geometry around the carbon atom the arrow is pointing to in the structure below?

a)

Bent

b)

Trigonal planar

c)

Trigonal pyramidal

d)

Tetrahedral

91.

Which of the following will exhibit metallic bonding?

a)

Zinc, Zn(s)

b)

CaCO₃(s), calcium carbonate

c)

C₃H₈(l), propane

d)

C, carbon (s)

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