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Chemistry Mid

Total questions: 55

Worksheet time: 5hrs 35mins

Name
Class
Date
1.

Which one of the following contributes to the charge, but does NOT contribute significantly to the mass of an atom?

a)

electrons

b)

nuclei

c)

photons

d)

neutrons

e)

protons

2.

Uranium exists in nature in the form of several isotopes; the different isotopes have different

a)

atomic numbers.

b)

charges.

c)

numbers of electrons.

d)

numbers of neutrons.

e)

numbers of protons.

3.

Which answer below best describes all atoms of a particular element?

a)

They possess the same number of electrons, the same atomic number, the same mass, but nothing else in common.

b)

They possess the same mass and the same chemical properties, but nothing else in common.

c)

They possess the same number of electrons, the same atomic number, the same chemical properties, but not necessarily the same mass.

d)

They possess the same chemical properties and the same mass, but nothing else in common.

e)

They possess the same atomic number and the same mass, but have nothing else in common.

4.

A neutral iodine atom has an atomic mass number = 131. Which description below fits this atom?

a)

39 protons, 78 neutrons, 39 electrons

b)

53 protons, 78 neutrons, 53 electrons

c)

52 protons, 79 neutrons, 54 electrons

d)

53 protons, 131 neutrons, 53 electrons

e)

54 protons, 131 neutrons, 54 electrons

5.

Which description below fits the 65Cu atom?

a)

29 protons, 65 neutrons, 29 electrons

b)

29 protons, 36 neutrons, 65 electrons

c)

29 protons, 36 neutrons, 31 electrons

d)

29 protons, 36 neutrons, 29 electrons

e)

31 protons, 34 neutrons, 29 electrons

6.

All of the following are alkali metals except

a)

Sr

b)

Na

c)

Fr

d)

Cs

e)

Rb

7.

Which element is a halogen?

a)

Te

b)

O

c)

Se

d)

Uuh

e)

I

8.

Each statement accurately describes the noble gases except for which one?

a)

They were once known as the inert gases.

b)

He, Ne, Ar, Kr, Xe, Rn, and Uuo are part of the group.

c)

Their heavier elements do react with other elements.

d)

They belong to group VIIIA (or 18).

e)

They contain at least one metalloid.

9.

The transition metals take up ___ periods of the periodic table.

a)

2

b)

3

c)

4

d)

1

e)

5

10.

In which family of elements does Ca belong?

a)

alkali metals

b)

alkaline earth metals

c)

halogens

d)

noble gases

e)

transition metals

11.

Some elements have properties that lie between true metals and true nonmetals. These elements are known as:

a)

metals

b)

nonmetals

c)

halogens

d)

alkaline earth metals

e)

metalloids

12.

Which metal is a liquid at room temperature (about 25oC)?

a)

hydrogen

b)

bromine

c)

tungsten

d)

mercury

e)

chromium

13.

Which of the following is not a property of metals?

a)

They have a shine called a metallic luster.

b)

They are good conductors of electricity.

c)

They are generally poor conductors of heat.

d)

They can be rolled into thin sheets.

e)

Some metals are quite hard, while some are soft.

14.

Classify the following three elements as a metal, metalloid, or nonmetal: P, Si, Al.

a)

P, metal; Si, metalloid; Al, nonmetal

b)

P, metal; Al, metalloid; Si, nonmetal

c)

Al, metal; P, metalloid; Si, nonmetal

d)

Si, metal; Al, metalloid; P, nonmetal

e)

Al, metal; Si, metalloid; P, nonmetal

15.

The formula for the phosphate ion is

a)

PO42-

b)

PO43-

c)

PO4-

d)

P2O4-

e)

P2O42-

16.

The correct formula for the carbonate ion is

a)

C2H3O2-

b)

C2O42-

c)

CO2-

d)

CO3-

e)

CO32-

17.

When barium metal reacts with chlorine gas, it forms an ionic compound, BaCl2. In the course of the reaction, each Cl atom

a)

loses one proton

b)

loses one electron

c)

gains one proton

d)

gains one electron

e)

loses one neutron

18.

Which formula is correct because it represents a known ionic compound?

a)

Be2Br4

b)

Ca2I2

c)

K2S

d)

Rb2Br

e)

Ca2S3

19.

How many protons, neutrons, and electrons are in the ion, 57Fe3+?

a)

27 protons, 30 neutrons, and 30 electrons

b)

26 protons, 31 neutrons, and 23 electrons

c)

29 protons, 28 neutrons, and 26 electrons

d)

26 protons, 31 neutrons, and 29 electrons

e)

25 protons, 32 neutrons, and 22 electrons

20.

The name of the compound Al(SO4)3 is

a)

there is no compound with that formula - it must be written incorrectly.

b)

aluminum sulfate

c)

aluminum trisulfate

d)

aluminum(III) sulfate

e)

aluminum sulfite

21.

What is the name for the compound CuBr2?

a)

copper(I) bromide(II)

b)

copper(II) bromide

c)

copper(II) bromite

d)

copper dibromide

e)

cuprous bromide

22.

Which is a correct name for the compound Hg2Cl2?

a)

dimercury dichloride

b)

mercuric chloride

c)

mercury(I) chloride

d)

mercury(II) dichloride

e)

there is no correct name, the formula should be HgCl

23.

What is the name for CuC2H3O2?

a)

copper(I) acetate

b)

carbon hydrocarbonate

c)

copper monocarbonate

d)

copper(I) oxalate

e)

dicarbon acetate

24.

The atomic mass of Mg is 24.305 u. How many moles of Mg are there in a 3.50 g sample of magnesium?

a)

0.0182 moles

b)

0.144 moles

c)

0.218 moles

d)

0.226 moles

e)

1.31 ×1023 moles

25.

A gas sample contains 16.0 g of CH4, 16.0 g of O2, 16.0 g of SO2, and 33.0 g of CO2. What is the total number of moles of gas in the sample?

a)

2.25 moles

b)

2.50 moles

c)

2.75 moles

d)

3.00 moles

e)

4.00 moles

26.

What is the percent, by mass, of tungsten in W(CH3)6?

a)

4.3819 %

b)

26.292 %

c)

67.083 %

d)

28.502 %

e)

35.722 %

27.

A compound has an empirical formula of CH2O. An independent analysis gave a value of 150.13 g for its molar mass. What is the molecular formula of the compound?

a)

C5H10O5

b)

C6H12O6

c)

C11H2O

d)

C6H6O8

e)

C9H10O2

28.

A 4.626 g sample of a hydrocarbon, upon combustion analysis, yielded 6.527 grams of water. The percent, by mass, of hydrogen in the hydrocarbon is therefore:

a)

14.11 %

b)

15.79 %

c)

41.09 %

d)

66.22 %

e)

85.89 %

29.

In a chemical reaction, C2H6O + SOCl2 ( C2H5Cl + H2SO3, when the equation is balanced the sum of the coefficients of the reactants and products should be

a)

4

b)

5

c)

6

d)

7

e)

8

30.

You are given the balanced chemical equation: C4H4 + 5 O2 ( 4 CO2 + 2 H2O. If 0.3618 moles of C4H4 are allowed to react with 1.818 moles of O2, and this is the only reaction which occurs, what is the maximum mass of water that could be produced?

a)

11.02 g

b)

13.04 g

c)

13.20 g

d)

19.64 g

e)

65.50 g

31.

The species shown below which has 24 electrons is

a)

a

b)

b

c)

c

d)

d

32.

When 1.20 moles C react with 1.20 moles O2, 2.40 moles CO2 are obtained

a)

True

b)

False

33.

.           In a chemical reaction, the best yield currently obtainable in any process is 99.5%.  ___ 

a)

True

b)

False

34.

In combustion analysis, a compound such as CH3(CH2)12CO2H, would have all its carbon atoms 

         converted to carbon dioxide._______

a)

True

b)

False

35.

A mole of oxygen, O2, and a mole of ozone, O3, do contain the same number of molecules. 
___ 

a)

True

b)

False

36.

A mole of naturally occurring Ne weighs more than a mole of O2.

a)

True

b)

False

37.

A sample of C7H5N3O4 contains 0.255 moles of hydrogen atoms.  This same sample also contains

 0.500 moles of oxygen atoms. _______

a)

True

b)

False

38.

The reaction between 1.12 moles of K and H2O, will produce more than 2.00 moles of KOH.  

          ____

a)

True

b)

False

39.

The number of protons in the nucleus of an atom, determines the order of elements in the periodic

table. ____

a)

True

b)

False

40.

Metalloids are capable of conducting an electric current. ____

a)

True

b)

False

41.

From left to right, across a row on the periodic table, there is a gradual change in properties from

nonmetallic to metallic properties. ____

a)

True

b)

False

42.

The name for ZnBr2, is zirconium bromide.  ___

a)

True

b)

False

43.

Bond formation tends to decrease the potential energy of the two atoms involved in forming the

         bond.____

a)

True

b)

False

44.

The lattice energy is the energy released if gaseous ions combine to form one mole of a solid ionic

          compound.____

a)

True

b)

False

45.

Compounds with negative heats of formation tend to be unstable with respect to decomposition into its elements.___

a)

True

b)

False

46.

The lattice energy of Al2O3 is greater than that for AlCl3, which implies that the melting point of

          Al2O3 should be greater than that of AlCl3. ___

a)

True

b)

False

47.

Based on the DHof data given, which compound is the most stable?

a)

a

b)

b

c)

c

d)

d

e)

e

48.

            Lithium fluoride has a lattice energy of -1033 kJ/mol.  In the ionic solid AB, A2+ has approximately the same radius as Li+, and B2- has approximately the same radius as F-. What is a reasonable estimate of the lattice energy of AB?

a)

a

b)

b

c)

c

d)

d

e)

e

49.

Which ionic solid is likely to have the largest exothermic lattice energy?

a)

KCl

b)

NaCl

c)

LiCl

d)

CsCl

50.

Which of the following solids is likely to have the largest exothermic lattice energy?

a)

            LiF

b)

NaCl

c)

AlCl3

d)

            Al2O3

51.

Which ionic solid is likely to have the smallest exothermic lattice energy?

a)

            KCl

b)

NaCl

c)

LiCl

d)

CsCl

e)

RbBr

52.

Which of the following solids is likely to have the smallest exothermic lattice energy?

a)

LiF

b)

NaCl

c)

AlCl3

d)

Al2O3

e)

CaCl2

53.

Based on the DHof data given below, which compound is the least stable

a)

H2S(g), -20.6 kJ/mol

b)

N2H4(g), +94.5 kJ/mol

c)

N2O(g), +81.6 kJ/mol

d)

Na2O2(g), -46.4 kJ/mol

 

54.

The attraction between positive and negative ions in an ionic compound is referred to as the

a)

ionic bond

b)

covalent bond

55.

Which cation is the most likely to form a stable ionic compound?

a)

Ca3+

b)

Ca2+

c)

Ca+

d)

O2+

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