Chemistry

Front 1

Classify each of the following properties of selected metals as a physical property or a chemical property.

A.Iron metal rusts in an atmosphere of moist air

B.Mercury metal is a liquid at room temperature

C.Nickel metal dissolves in acid to produce a light green solution

D.Potassium metal has a melting point of 63 deg

Back 1

chemical, physical, chemical, physical

Front 2

Classify each of the following as matter or energy (non-matter).

A.Water

B.Electricity

C.Air

Back 2

matter, non-matter, matter

Front 3

All heterogeneous mixtures must contain three or more substances.

Back 3

False

Front 4

Pure substances cannot have a variable composition.

Back 4

true

Front 5

Substances maintain their identity in a heterogeneous mixture, but not in a homogeneous mixture.

Back 5

False

Front 6

Assign each of the following descriptions of matter to one of the following categories: element, compound, or mixture.

A.One substance present, three elements present.

B.Two elements present, composition is variable.

C.One substance present, one phase present, substance cannot be decomposed using chemical means.

Back 6

compound, mixture, element

Front 7

* Select the diagram or diagrams that represent(s) a pure substance.

Back 7

I, IV

Front 8

Write the name of the metric system prefixes associated with each of the following mathematical factors.

a.0.001 or 10-3

b.1000 or 103

c.0.01 or 10-2

d.0.1 or 10-1

Back 8

milli, kilo, centi, deci

Front 9

Indicate whether the number in the following statement is an exact or an inexact number:

A classroom contains 32 chairs. The number 32 is an (exact, inexact) number.

Back 9

exact

Front 10

Determine the number of significant figures in each of the following measured values.

A.65,400

B.76.010

Back 10

5,5

Front 11

Indicate to what decimal position a reading should be recorded for a measurement made with a 100-mL volumetric cylinder with a smallest scale marking of 10 mL.

Back 11

nearest 1 mL

Front 12

Round off the following measured value to three significant figures;

456,455.

Back 12

456,000

Front 13

What volume of water, in gallons, would be required to fill a 25-mL container?

Back 13

.0066 gallons

Front 14

Acetone, the solvent in nail polish remover, has a density of 0.791 g/mL. What is the volume, in milliliters (mL), of 20.0 g of acetone?

Back 14

20.0/.791= 25.3

Front 15

An oven for baking pizza operates at approximately 525oF. What is this temperature in degrees Celsius?

Answer: __________ C

Back 15

5/9(525-32)=274

Front 16

True or False: The number of nucleons present in the nucleus is equal to the number of electrons present outside the nucleus.

Back 16

False

Front 17

Determine the number of protons , neutrons , and electrons present for an atom that has an Mass number = 18 and Z = 8.

Back 17

Protons: 8 Neutrons:10 Electrons: 8

Front 18

Characterize each of the following pairs of atoms as containing (1) the same number of neutrons, (2) the same number of protons, (3) the same number of nucleons, or (4) the same total number of subatomic particles.

(a) 137C and 136N

(b) 3717Cl and 3618Ar

(c) 3517Cl and 3717Cl

(d) 188O and 199F

Back 18

same number of nucleons, same number of subatomic particles, same number of protons, same number of neutrons

Front 19

Which of these properties would also be the same for the second-most-abundant isotope of the element?

A.Mass number is 70

B.31 electrons are present

C.Isotopic mass is 69.92 amu

D.Isotope reacts with chlorine to give a green compound

Back 19

not the same, same, not the same, same

Front 20

Calculate the atomic mass for the following element using the given data for the percentage abundance and mass of each isotope:

Lithium: 7.42% 6Li (6.01 amu) and 92.58% 7Li (7.02 amu)

Back 20

6.95

Front 21

Based on periodic table position, select the two elements from the following set of elements that would be expected to have SIMILAR chemical properties.

19K, 29Cu, 37Rb, 41Nb

Back 21

19K, 37Rb

Front 22

This is a vertical arrangement of elements in the periodic table.

Back 22

Group

Front 23

The properties of the elements repeat in a regular way as atomic numbers increase.

Back 23

periodic law

Front 24

This is a horizontal arrangement of elements in the periodic table

Back 24

Period

Front 25

Carbon is the first member of this arrangement.

Back 25

group

Front 26

Which of the following units can contain a maximum of two electrons?

A. electron orbital

B.electron shell

C.electron subshell

Back 26

electron orbital

Front 27

Give the maximum number of electrons that can occupy the 4p subshell.

Back 27

6 electrons

Front 28

On the basis of the total number of electrons present, identify the element whose electron configuration is:

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

Back 28

As

Front 29

Indicate whether the elements represented by the given pairs of electron configurations have similar chemical properties.

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

Back 29

similar

Front 30

Classify the following by whether they are, or tend to form cations or anions:

Br

positive charged

Group IIA

metals

Group VIIA

nonmetals

more electrons than protons

Back 30

anion, cation, cation, cation, anion, anion, anion

Front 31

How many valence electrons do atoms with the following electron configuration have?

1s2 2s2 2p6 3s2 3p1

Back 31

3

Front 32

Which of the following are valid Lewis-Dot Structures for the neutral atoms indicated?

Back 32

a, c

Front 33

Select all the true statements:

1. The Cl- and Br- ions have the same number of electrons.
2. Anions carry a positive charge.
3. When an atom gains an electron, it becomes a cation.
4. The K+ ion is formed when a potassium atom loses one electron.
5. The Fe2+ and Fe3+ ions have the same number of protons.
6. The Cu+ and Cu2+ ions have the same number of electrons.

Back 33

4, 5

Front 34

which of the following is NOT a fixed charged metal?

Ni,Ag, Zn,Al,Li

Back 34

Ni

Front 35

The attraction between positive and negative ions make an/a _____________bond.

Back 35

ionic

Front 36

An ion containing 16 protons, 16 neutrons, and 18 electrons has what charge?

Back 36

-2

Front 37

How many cesium ions would normally join with nitride in forming cesium nitride?

Back 37

3

Front 38

What is the best chemical formula for a compound formed from aluminum and sulfur?

Back 38

AL3S2

Front 39

What is the correct name for Ca3(PO4)2?

Back 39

Calcium Phosphate

Front 40

What is the best chemical formula for chromium (III) oxide?

Back 40

Cr2O3

Front 41

What is the name for the compound Fe2(SO4)3

Back 41

Iron (III) Sulfate

Front 42

What is the name for a compound formed from Gallium and Sulfur.

Back 42

Gallium sulfide

Front 43

Methyl Chloride has the chemical formula CH3Cl. How many non-bonding electrons must be shown in the Lewis structure of Methyl Chloride?

Back 43

6

Front 44

The toxic gas hydrogen cyanide has the formula HCN. Which of the following is a correct description of hydrogen cyanide?

HCN has only single bonds

HCN has two double bonds

none of these are correct

HCN has one double bond

HCN has one triple bond

Back 44

HCN has one triple bond

Front 45

What is the IUPAC name of NO2?

Back 45

nitrogen dioxide

Front 46

Which of the following molecules is polar?

(a) CH3Cl

(e) none of these

(d) both 1 and 2

(c) CCl4

(b) HCN

Back 46

Both a and c

Front 47

Which of the following is true about a molecule which contains two polar bonds which have the same degree of polarity?

A.It will never be polar

B.It will always be polar

C.It will only be polar if it is bent

D.It will only be polar if it is linear

Back 47

it will only be polar if it is bent

Front 48

Determine the total number of non-bonding electrons

Back 48

6

Front 49

Back 49

trigonal pyramidal

Front 50

Which type of bond exists in each of these compounds?

KCl,BCl3, P4, CO

Back 50

ionic bonds

polar covalent bonds

nonpolar covalent bonds

polar covalent bonds

Front 51

Balance the equation; ___H2 + ___O2 --> ___H2O

Back 51

2,1,2

Front 52

Balance the equation: ___ C6H14 + ___ O2 --> ___ CO2 + ___H2O

Back 52

2,19, 12,14

Front 53

Define molar mass

Back 53

the mass, in grams, of one mole of a substance

Front 54

Exactly 1 mole of H3PO4 contains how many moles of H, P, and O?

Back 54

H=3 P=1 O=4

Front 55

How many moles of MgS2O3 are in 207 grams of the compound?

_________ moles MgS2O3

*Use molar mass

Back 55

1.52

Front 56

How many moles of hydrogen atoms are in 3.10 moles of ammonium sulfate?

_______ moles H atoms

Back 56

24.8

Front 57

How many grams of phosphorus are in 3.40 mol of copper(II) phosphate?

_________ grams P

Back 57

211

Front 58

The combustion of propane may be described by the chemical equation:

C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(g)

How many grams of O2(g) are needed to completely burn 66.9 grams of C3H8(g)? _______grams of O2(g)

Back 58

243

Front 59

In a chemical reaction, exactly 2 mol of substance A react to produce exactly 3 mol of substance B.

2A 3B

How many grams of substance B are produced when 81.0 g of substance A reacts? The molar mass of substance A is 27.0 g/mol and the molar mass of substance B is 54.0 g/mol.

A.Convert the mass of A to moles of A = ________

B.Convert the number of moles of A to the number of moles of B = __________

C.Convert the number of moles of B to grams of B = ________

Back 59

A. 3

B.4.5

C.243

Front 60

How many molecules are present in 2.00 moles of CaSO4?

Back 60

2 × 6.02 10^23

Front 61

The reaction between hydrochloric acid and aluminum produces hydrogen gas and aluminum chloride. The balanced reaction equation is given below. How many moles of H2 can be obtained when 4.40 mol HCl reacts with an excess of Al?

6HCl + 2Al 3H2 +2AlCl3_____________ moles H2

Back 61

2.20

Front 62

This state is characterized by the lowest density of the three states.

Back 62

gas

Front 63

This state is characterized by an indefinite shape and high density.

Back 63

liquid

Front 64

Temperature changes significantly influence the volume of this state.

Back 64

gas

Front 65

Pressure changes influence the volume of this state more than the other two states.

Back 65

gas

Front 66

In this state constituent particles are less free to move around than in other states.

Back 66

solid

Front 67

An adult human breathes in approximately 0.500 L of at at 32.0 C and 1.00 atm pressure with every breath. What would this "breath volume" be at the same pressure if the temperature drops to 21.0 C?

Breath volume = ___________ L

*Charles law

Back 67

.482

Front 68

Back 68

Tetrahedral

Front 69

Back 69

linear

Front 70

Back 70

Bent

Front 71

Determine the total number of non-bonding electrons

Back 71

4

Front 72

Determine the total number of non-bonding electrons

Back 72

6

Front 73

If an ideal gas has a pressure of 8.55 atm, a temperature of 142 C, and has a volume of 95.21 Liters, how many moles of gas are in the sample?

Back 73

23.9

Front 74

Which of the following statements regarding phase changes are true? Select all that apply.

A.Freezing converts a gas to a liquid

B.Deposition converts a gas to a solid

C.Melting converts a solid to a liquid

D.Sublimation converts a gas to a solid

Back 74

b,c

Front 75

For liquids, which of the following factors affect vapor pressure?

A.intermolecular forces

B.temperature

C.surface area

D.volume

E.humidity

Back 75

a,b

Front 76

Which of the following affect the strength of London forces?

(a) number of electrons

(b) size

(c) shape

(d) all of these

(e) none of these

Back 76

D-all of these

Front 77

Which of the following is true of the vapor pressure of a liquid?

A.the vapor pressure of all liquids are the same

B.the vapor pressure of a liquid is an equilibrium pressure

C.the vapor pressure of a liquid is independent of temperature

D.the vapor pressure of a liquid can be measured in an open container

E.none of these

Back 77

b

Front 78

Which of the following is necessary for a molecule to engage in hydrogen bonding?

(a) there must be a hydrogen atom covalently bonded to a nitrogen atom
(b) there must be a hydrogen atom covalently bonded to a oxygen atom
(c) either (a) or (b)
(d) neither (a) nor (b)

Back 78

c

Front 79

Which of the following molecules do not involve hydrogen bonding.

A.NH3

B.HF

C.H2O

D.CH4OH

E.NF3

Back 79

E-NF3

Front 80

The process of boiling is a form of evaporation.

Back 80

True

Front 81

The boiling point of a liquid heated in an open container is determined by atmospheric pressure.

Back 81

True

Front 82

The normal boiling point of a liquid is the temperature at which it boils when the liquid is at sea level.

Back 82

True