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Midterm Exam Review

Total questions: 89

Worksheet time: 45mins

Name
Class
Date
1.

Which two of these states of matter fill the container?

a)

Solid

b)

Liquid

c)

Gas

2.

For a heterogeneous mixture, what experimental technique do you use to remove solids?

a)

Chroatography

b)

Infrared Spectroscopy

c)

Filtration

d)

Distillation

3.

During distillation a liquid is ___________ to produce a vapor that is then condensed into a liquid.

a)

Filtered

b)

Boiled

c)

Cooled

d)

Mixed

4.

The simplest form of matter that has a unique set of properties.

a)

Compound

b)

Element

c)

Mixture

d)

Gas

5.

Can you break a compound into simpler substances?

a)

Yes

b)

No

6.

Who do you think is the cooler teacher?

a)

Mr. Tham

b)

Mr. Fursdon-Welsh

c)

Any other teacher at YHIS!

7.

What experimental setup is this?

a)

Filtration

b)

Distillation

c)

Chromatography

d)

Scanning Electron Microscope

8.

A substance that contains two or more elements chemically combined in a fixed proportion.

a)

Element

b)

Compound

c)

Mixture

d)

Nucleus

9.

The following are all examples of ____________


Burn, rot, corrode, decompose

a)

Chemical Changes

b)

Physical Changes

c)

Reactions

d)

Mixtures

10.

What clues could tell us that a chemical change has taken place? (select all possible answers)

a)

Change in color

b)

Formation of a precipitate

c)

Transfer of energy

d)

Production of a gas

11.

What is this number in scientific notation?


6,926,300,000

a)

6.9263×10−96.9263\times10^{-9}

b)

6.9263×1096.9263\times10^9

c)

6.9×1096.9\times10^9

d)

6.9263×10116.9263\times10^{11}

12.

To multiply numbers written in scientific notation, multiply the coefficients and (a)   the exponents.

13.

If you want to add or subtract numbers expressed in scientific notation and you are not using a calculator, then the exponents must be the _____.

a)

same

b)

different

14.

Which of these has bad accuracy and good precision?

a)
b)
c)
15.

How many significant figures?


24.7 meters


0.743 meter


714 meters

a)

2

b)

3

c)

4

16.

How many significant figures?


7003 meters

a)

4

b)

3

c)

5

17.

How many significant figures?


0.42 meter

a)

3

b)

1

c)

2

18.

How many significant figures?


9.000 meters

a)

4

b)

1

c)

3

19.

How many significant figures?


27,210 meters

a)

5

b)

4

c)

6

20.

Round this number to two significant figures:


3675

a)

3680

b)

3700

c)

3600

d)

3670

21.

In general, a calculated answer cannot be more precise than the ________ precise measurement from which it was calculated.

a)

Least

b)

Most

22.

 massvolume= ?\frac{mass}{volume}=\ ?  

a)

Weight

b)

Density

c)

Ratio

23.

Which science subject is the coolest?

a)

Chemistry

b)

Physics

c)

Biology

d)

All of them!

24.

Protons have a (a)   charge.

25.

The nucleus contains protons and (a)   .

26.

Atomic Number: Elements are different because they contain different numbers of _________.

a)

electrons

b)

protons

c)

mass

d)

neutrons

27.

Atoms are electrically neutral so the number of electrons in an atom equals the number of protons.

a)

True

b)

False

28.

The total number of protons and neutrons in an atom is called the ____ number.

a)

atomic

b)

mass

c)

proton

d)

periodic

29.

Isotopes are atoms that have the same number of protons but different numbers of (a)   .

30.

The atomic mass of an element is a _________ average mass of the atoms in a naturally occurring sample of the element.

a)

weighted

b)

total

c)

mean

31.

Carbon-12 has six protons and six neutrons. It has an atomic mass of (a)   .

32.

What is the correct electron configuration of a sulfur atom?

a)

1s22s22p43s23p6

b)

1s22s22p63s23p3

c)

1s22s22p63s23p4

d)

1s22s22p63s63p2

33.

λ is ________________

a)

frequency

b)

wavelength

c)

wave

d)

period

34.

The red wave has a higher frequency than the red wave

a)

True

b)

False

35.

The SI unit for frequency is?

a)

meters/second

b)

meters

c)

hertz

d)

seconds

36.

Energy is released as a light wave when an electron _____ an energy level

a)

emits

b)

drops

c)

gains

37.

According to the photoelectric effect, when light below the threshold frequency is shone on a metal it will not eject an electron.

a)

True

b)

False

38.

Some elements on the periodic table have the same emission spectra

a)

True

b)

False

39.

Elements in the periodic table are arranged in order of increasing _______________

a)

Reactivity

b)

Radioactivity

c)

Atomic number

40.

Nitrogen, sulfur, phosphorus, bromine and carbon are examples of non metals.

a)

True

b)

False

41.

In general, atomic size ____________ as you go down a group, and ___________ from left to right across a period.

a)

Increases/Increases

b)

Increases/Decreases

c)

Decreases/Increases

d)

Decreases/Decreases

42.

An ion with a positive charge is called a (a)  

43.

An ion with a negative charge is called an (a)  

44.

Group 1 and Group 2 metals tend to form anions.

a)

True

b)

False

45.

The energy required to remove an electron from an atom is called ______________

a)

Electron affijnity

b)

Ionization energy

c)

Electronegatvity

46.

In general, ionization energy ____________ as you go down a group, and ___________ from left to right across a period.

a)

Increases/Increases

b)

Increases/Decreases

c)

Decreases/Increases

d)

Decreases/Decreases

47.

Second ionization energies are always greater than first ionization energies.

a)

True

b)

False

48.

Cations are always _________ than their corresponding neutral atom.

a)

smaller

b)

larger

49.

______________ is the ability of an atom of an element to attract electrons when the atom is in a compound.

a)

Electron affijnity

b)

Ionization energy

c)

Electronegatvity

50.

In general, electronegatvity ____________ as you go down a group, and ___________ from left to right across a period.

a)

Increases/Increases

b)

Increases/Decreases

c)

Decreases/Increases

d)

Decreases/Decreases

51.

Select the common properties of non-metals (select 4 answers)

a)

Brittle

b)

Poor conductors of heat

c)

Poor conductors of electricity

d)

Mostly gases and solids

e)

Malleable

52.

Electrons in the highest occupied energy level of an element’s atoms are called?

a)

Anions

b)

Valence electrons

c)

Cations

d)

Ionic bonding

53.

The __________ states that in forming compounds, atoms tend to achieve the electron configuration of a noble gas.

a)

octet rule

b)

anion

c)

alloy

d)

cation

54.

The ionic compound, Sodium Chloride (NaCl) has a neutral charge?

a)

True

b)

False

55.

Ionic compounds are often brittle

a)

True

b)

False

56.

The structure of metals is positive cations floating in a sea of _____________.

a)

protons

b)

electrons

c)

neutrons

d)

atoms

57.

Metals are poor conductors of heat and electricity.

a)

True

b)

False

58.

This an example of:

a)

an allotrope

b)

a metallic bond

c)

an ionic bond

d)

an electron dot structure

59.

How many electrons does a bond (line) in an electron dot structure represent?

(a)  

60.

Bonding in ozone is an example of a __________________.

a)

metallic bonding

b)

ionic bonding

c)

a resonance structure

d)

a coordinate bond

61.

In a polar covalent bond, there is a slight negative charge on the _______ electronegative atom.

a)

more

b)

less

62.

This molecule has bond dipoles and a molecular dipole.

a)

True

b)

False

63.

How will a polar molecule orient itself in an electric field (between two electrically charged plates)?

a)

The positive end of the dipole towards the negative plate and the negative end of the dipole towards the positive plate.

b)

The positive end of the dipole towards the positive plate and the negative end of the dipole towards the negative plate.

64.

This is an example of:

a)

a dipole-dipole interaction

b)

an ionic bond

c)

dispersion forces

d)

an ion-dipole interaction

65.

This is an example of:

a)

An ionic bond

b)

A covalent bond

c)

A metallic bond

d)

A coordinate bond

66.

This is an example of:

a)

a dipole-dipole interaction

b)

an ionic bond

c)

dispersion forces

d)

an ion-dipole interaction

67.

Hydrogen "bonds" are a special type of dipole-dipole interaction when hydrogen atoms are bonded to which three of the following atoms:

a)

Silicon

b)

Nitrogen

c)

Fluorine

d)

Carbon

e)

Oxygen

68.

This is an example of:

a)

a dipole-dipole interaction

b)

an ionic bond

c)

dispersion forces

d)

an ion-dipole interaction

69.

The only intermolecular forces present with noble gases and alkanes (such as methane) are:

a)

ion-dipole interactions

b)

dispersion forces

c)

dipole-dipole interactions

d)

ionic bonding

70.

The greater the amount of intermolecular forces present, the lower the melting/boiling points in the substance.

a)

True

b)

False

71.

Covalent bonds are stronger than all the intermolecular forces.

a)

True

b)

False

72.

What is the charge of a sodium ion?

a)

-2

b)

+1

c)

-1

d)

+2

73.

What is the charge of a chloride ion?

a)

-2

b)

+1

c)

-1

d)

+2

74.

How many valence electrons does magnesium have?

a)

1

b)

2

c)

3

d)

4

75.

The prefix poly- means:

a)

Parrot

b)

Few

c)

Chemistry

d)

Many

76.

Polyatomic ions contain covalent bonds and are able to form ionic bonds.

a)

True

b)

False

77.

What is the NH4+ ion called?

a)

Sulphite

b)

Sulfate

c)

Ammonium

d)

Carbonate

78.

What is the CO32- ion called?

a)

Sulphite

b)

Sulfate

c)

Ammonium

d)

Carbonate

79.

What is the molecular formula for the sulfate ion?

a)

SO42-

b)

OH-

c)

PO43-

d)

NO3-

80.

What is the molecular formula for the phosphate ion?

a)

SO42-

b)

OH-

c)

PO43-

d)

NO3-

81.

Ca3P2

What is the name of this molecule?

a)

Calcium diphosphide

b)

Calcium phosphorus

c)

Calcium phosphide

d)

Calcium potassiumide

82.

Hg2Cl2

What is the name of this molecule?

a)

Hergium chloride

b)

Mercury chlorine

c)

Dimercury dichloride

d)

Mercury (I) chloride

83.

CaCO3

What is the name of this molecule?

a)

Calcium carbonate

b)

Calcium carbide

c)

Calcium carbon trioxide

d)

Carbon Carbonate

84.

What is the formula for ammonium phosphate?

a)

NH4PO4

b)

NH4(PO4)3

c)

(NH4)3PO4

d)

AmPh4

85.

Sr(NO2)2

What is the name of this molecule?

a)

Strontium nitrate

b)

Tin nitrate

c)

Strontium nitrite

d)

Monostrontium binitrite

86.

SiS2

What is the name of this molecule?

a)

Monosilicon disulfide

b)

Silicon disulfide

c)

Silicon sulfide

d)

Monosilicon sulfide

87.

HCl is an acid

a)

True

b)

False

88.

HI

What is the name of this molcule?

a)

Iodine hydroxide

b)

Hydrobromic acid

c)

Iodic acid

d)

Hydroiodic acid

89.

Cl2O7

What is the name of this molecule?

a)

Dichlorine hepatoxide

b)

Chlorine oxide

c)

Dichlorine heptoxide

d)

Dichlorine pentoxide

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