wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Year end final

Total questions: 100

Worksheet time: 50mins

Name
Class
Date
1.

Which of the following elements has the lowest electronegativity?

a)

Lithium

b)

Bromine

c)

Carbon

d)

Oxygen

2.

what is the activation energy for the reverse reaction of the following:

a)

35 kJ

b)

25 kJ

c)

40 kJ

d)

15 kJ

3.

The Bohr model of the atom is similar to

a)

central ball with lighter balls connected

b)

a basketball

c)

plum pudding

d)

solar system

4.

Which of the following processes will give a negative value of ΔH?

a)

H2O (s) → H2O(l)

b)

H2O(l) → H2O (s)

c)

CO2 (s) → CO2 (g)

d)

NH3(l) → NH3 (g)

5.

The tendency to gain electrons-------as you move down a column on the periodic table

a)

remains the same

b)

increases

c)

decreases

d)

increases, then decreases

6.

What is the condensation point of the following substance?

a)

92

b)

30

c)

120

d)

58

7.

The pressure of gas will----when the volume is decreased and will----when the absolute temperature is decreased.

a)

decrease, increase

b)

increase, decrease

c)

increase, increase

d)

decrease, decrease

8.

Atoms of a covalent bond are held together by the attraction.....

a)

between two nuclei

b)

for 2 shared electrons

c)

of protons and electrons

d)

between two charged ions

9.

The outer electron configuration of an alkali metal has

a)

1 electron in the s orbital

b)

2 electrons in the s orbital

c)

1 electron in the p orbital

d)

2 electrons in the p orbital

10.

Which of the following is a weak electrolyte?

a)

HClO4

b)

HClO3

c)

HClO2

d)

NaOH

11.

Trends in the periodic table indicate that the element with the greatest ionization energy is in which of the following period and group?

a)

Period 7, group 2

b)

Period 2, group 1

c)

Period 6, group 17

d)

Period 1, group 18

12.

What is the hybridization on the carbon of the methane molecule?

a)

sp

b)

sp2

c)

sp3

d)

sp4

13.

Which of the following reactions have a negative entropy change? I. 2H2 (g) + O2 (g)→2H2O(l)

II. 2NH3 (g) → N2(g) + 3H2(g)

III. Ca(s) + Cl2(g) → 2CaCl2(s)

a)

I only

b)

II only

c)

I and III

d)

II only

14.

What phase change occurs if pressure is increased at point "y" in the diagram...

a)

melting

b)

freezing

c)

condensation

d)

vaporization

15.

What is the value of the self ionization constant of water?

a)

55.4

b)

1.00 x 10-14

c)

14

d)

1.00 x 10-7

16.

What is the electron configuration of the Fluoride ion?

a)

1s2 2s2 2p6 3s2

b)

1s2 2s2 2p6

c)

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

d)

1s2 2s2 2p6 3s2 3p5

17.

The true volume of a real gas is smaller than that calculated from the ideal gas law equation under low temperatures. This occurs because the ideal gas equation does NOT correct for:

a)

the finite volume of molecules

b)

the mass of molecules

c)

the attraction between molecules

d)

the shape of molecules

18.

A very high value of the equilibrium constant for a reaction indicates that

a)

equilibrium has been reached

b)

reactants are favored

c)

products are favored

d)

equilibrium has shifted

19.

What subatomic particle determines the identity of an element?

a)

neutrons

b)

protons and quarks

c)

protons

d)

electrons

20.

What type of bond would you expect between an iron and an oxygen atom?

a)

covalent

b)

reactive

c)

metallic

d)

ionic

21.

What is the concentration of OH- ions in pure water?

a)

1.00 x 10-14 M

b)

zero

c)

1.00 x 10-7 M

d)

8.00 M

22.

Which liquid has the lowest vapor pressure?

a)

Na2CO3

b)

K2O

c)

CaCO3

d)

Al2(CO3)2

23.

What is the formula for Lead (II) chromate?

a)

PbCO4

b)

PbCrO

c)

PbCrO4

d)

PbCrO7

24.

Why did J.J. Thomson reason that electrons must be a part of the atoms of all elements?

a)

Cathode rays are negative

b)

an electron is very small, so it must be everywhere

c)

cathode rays can be deflected by magnets

d)

the charge/mass ratio was the same regardless of gas used

25.

Which of the following is not a property of an ionic compound:

a)

low boiling point

b)

electrolytes

c)

formed by ions

d)

hard

26.

A mole is 6.02 x 1023 atoms of ------ grams of -------isotope

a)

1 g, H-1

b)

18g, H2O

c)

12 g, C-12

d)

16 g, O-16

27.

When an electrons moves from a lower to a higher energy level, energy is

a)

released

b)

absorbed

c)

created

d)

changed

28.

If the temperature of the equilibrium system: X + Y ↔ XY + 25 kJ, decreases....

a)

[X] decreases and [XY] decreased

b)

concentrations will stay the same

c)

[X] increases and [XY] decreases

d)

[X] decreases and [XY] increases

29.

The lines in the emission spectrum of hydrogen result from------

a)

protons given off when hydrogen burns

b)

electrons given off when hydrogen burns

c)

energy given off when hydrogen burns

d)

decomposing hydrogen atoms

30.

In a horizontal row, the ionization energy tends to ----- with increasing atomic number

a)

remain the same

b)

increase

c)

decrease

d)

increase, then decrease

31.

Which of the following elements has the smallest first ionization energy?

a)

Potassium

b)

calcium

c)

magnesium

d)

sodium

32.

What is the bond angle in a water molecule?

a)

180

b)

120

c)

104.5

d)

109.5

33.

The molecualr gemoetry of PF3 molecule is ----- and this molecule is -----

a)

trigonal planar, nonpolar

b)

trigonal planar, polar

c)

trigonal pyramid, polar

d)

trigonal pyramid, nonpolar

34.

What is the formula for a compound formed by thyocyanate?

a)

BaSCN

b)

BaCN

c)

Ba(SCN)2

d)

Ba(CN)2

35.

The least reactive elements are those of the

a)

metals

b)

transition elements

c)

nonmetals

d)

noble gases

36.

Name the compound: Ni(ClO3)2

a)

nickle chlorite

b)

nickle chlorate

c)

nickle (II) chlorate

d)

nickle (I) chlorate

37.

The molecular geometry of BF3 molecule is---- and this molecule is -----.

a)

trigonal planar, polar

b)

trigonal planar, nonpolar

c)

trigonal pyramid, polar

d)

trigonal pyramid, nonpolar

38.

What is the pH of a 1 x 10-4 M HCl solution?

a)

11

b)

1

c)

4

d)

10

39.

Which of the following substance has the lowest boiling point?

a)

PH3

b)

NH3

c)

H2S

d)

CH4

40.

Name the compound: Fe(NO2)2

a)

Iron nitrate

b)

Iron nitrite

c)

Iron (I) nitrate

d)

Iron (II) nitrite

41.

What is true of isotopes? They have the....

a)

same nucleous but different electorn cloud

b)

same number of protons but different number of neutrons

c)

same number of neutrons but differnet number of electrons

d)

same number of protons but different number of electrons

42.

Which of the following is an example of a network covalent solid?

a)

CaCO3

b)

NaCl

c)

Sugar

d)

SiO2

43.

if the pressure on the reaction N2(g) + O2(g) ↔ 2NO(g) at eqiulibrium is increased,

a)

The quantities of all substances do not change

b)

the quantity of NO decreases.

c)

teh quantity of N2 decreases

d)

the quantity of NO increases

44.

name the compound Zn3(PO4)2

a)

Zinc (III) phosphate

b)

Zinc phosphate

c)

Zinc (II) phosphate

d)

Zinc phospide

45.

How many neutrons are present in the isotope: 26X12

a)

12

b)

26

c)

38

d)

14

46.

How does atomic radius change form top to bottom in a group in the periodic table?

a)

it increases

b)

it decreases

c)

it increases then decreases

d)

it decreases, then increases

47.

The products of a combustion reaction do NOT include-----

a)

water

b)

carbon dioxide

c)

hydrogen

d)

carbon monoxide

48.

Teh products of neutralization reaction include-----

a)

salt and sugar

b)

salt and water

c)

acid and base

d)

acid and salt

49.

For the alkaline-earth metals, atoms with the smallest radii have the

a)

largest volumes

b)

largest atomic number

c)

highest ionization energy

d)

most mass

50.

In a double bond, two atoms share a total of ----- electrons.

a)

six

b)

two

c)

four

d)

three

51.

Which of the following isotopes has the same number of neutrons as Phosphorous-31

a)

Sulfur-32

b)

Phosphorous-32

c)

Silicon-28

d)

Silicon-29

52.

A solution whose pH is 4

a)

is always basic

b)

is always acidic

c)

is always neutral

d)

might be neutral or acidic

53.

A conjugate base is the species that

a)

is formed by the addition of a proton to a base

b)

remains after an acid has given up a proton

c)

is formed by the addition of a proton

d)

remains after a base has given up a proton

54.

A dissolved solute that does NOT form ions is

a)

a strong electrolyte

b)

a weak electrolyte

c)

a nonelectrolyte

d)

insoluble

55.

In a an acid-base titration, equivalent quantities of hydronium ions and hydroxide ions are present

a)

at the equivalence point

b)

at the end point

c)

at the midpoint

d)

at the beginning

56.

What is the change in enthalpy for the reaction....

a)

1

b)

2

c)

3

d)

4

57.

The hybridization around the SF6 molecule is ----- and the molecule is -----.

a)

sp2, polar

b)

sp3d, polar

c)

sp3d, nonpolar

d)

sp3d2, nonpolar

58.

What type of bond would you expect between two chlorine atoms?

a)

metallic

b)

nonmetallic

c)

ionic

d)

Covalent

59.

ionic compounds are brittle because the strong attractive forces...

a)

keep the surface dull

b)

allow the layers to shift easily

c)

cause the compound to vaporize easily

d)

hold the layers in fixed positions

60.

If teh system 2CO(g) + O2(g) ↔ 2CO2(g) has come to equilibrium and then more CO2 is added,

a)

both [CO] and [O2] increase

b)

[CO] increases and [O2] decreases

c)

[CO] decreases and [O2] increases

d)

both [CO] and [O] decreases

61.

Which of the following processes is endothermic?

a)

CO2(g) → CO2(s)

b)

H2O(g) → H2O (l)

c)

H2O(l) → H2O (s)

d)

NH3(l) → NH3(g)

62.

What is the freezing point of the following substance?

a)

30

b)

58

c)

92

d)

120

63.

Which of the following is soluble in water?

a)

NH3

b)

CF4

c)

C6H6

d)

BH3

64.

The letter "p" in teh symbol 4p3 indicates the ----

a)

speed of electron

b)

orbital shape

c)

spin of electron

d)

energy level

65.

Electronegativity------------as you go right across a row

a)

increases

b)

decreases

c)

remain the same

d)

increase, then decreases

66.

Which of these intermolecular forces accounts for the nonpolar parafin wax existing as a solid at room temperature?

a)

hydrogen bonding

b)

Dispersion forces

c)

dipole-dipole

d)

ion-dipole

67.

Which of the following is capable of hydrogen bonding?

a)

methane

b)

ammonia

c)

salt

d)

diamond

68.

The correct Lewis structure for a fluorine atom in a molecule of F2 shows

a)

one shared pair of electrons

b)

two shared pair od electrons

c)

no shared apir of electrons

d)

three shared pairs of electrons

69.

consider the reaction: N2(g) + 3H2(g) ↔ 2NH3 (g). what is the effect of decreasing the volume on the reaction?

a)

The equilibrium shifts right

b)

The equilibrium shifts left

c)

The equilibrium does not shift

d)

The equilibrium is terminated

70.

Of the compounds below, only---- is NOT an electrolyte.

a)

MgO

b)

H2O

c)

HCl

d)

NaOH

71.

What is the formula for aluminum sulfate?

a)

AlS3

b)

AlSO3

c)

Al2(SO4)3

d)

AlSO4

72.

Which diagram in the picture, shows the appropriate catalyst in a chemical reaction?

a)

A

b)

B

c)

C

d)

D

73.

The molecular geometry of the left-most Carbon in the molecule is...

a)

trigonal pyramid

b)

trigonal planar

c)

tetrahedral

d)

linear

74.

A solution with a pH of 10 is

a)

Always acidic

b)

Always Basic

c)

Always neutral

d)

might be acidic, basic or neutral

75.

Arrange the following gases in order of increasing average molecular speed at 25oC. Cl2, O2, F2, N2

a)

F2 < O2 < N2< Cl2

b)

Cl2< F2 < O2 < N2

c)

Cl2 < F2 < N2 < O2

d)

N2 < F2 < Cl2 < O2

76.

What is the pH of a 1 x 10-5 M NaOH solution?

a)

5

b)

9

c)

3

d)

11

77.

Why does H2O have a higher boiling point than SeH2

a)

SeH2 has hydogen bonding and H2O does not

b)

H2O has hydrogen bonding and SeH2 does not

c)

H2O is bend and SeH2 is not

d)

SeH2 is bent and H2O is not

78.

Which is true for the following reaction? A+ B → C+ D ΔH=+557kJ

a)

it is endothermic

b)

it is exothermic

c)

it is releasing heat

d)

it is releasing entropy

79.

The pH of a solution is 9 What is the H3O+ concentration?

a)

9 M

b)

5 M

c)

1 x 10-9 M

d)

1 x 10-5 M

80.

Decreasing the temperature of an ideal gas from 80 K to 40 K causes the average kinetic energy to

a)

decrease by a factor of two

b)

increase by a factor of two

c)

increase by a factor of four

d)

decrease by a factor of 4

81.

The chart below shows the relationship between ionization energy and atomic number. The letter on the chart for the noble gases is

a)

Z

b)

Y

c)

X

d)

W

82.

In the diagram below, which labeled arrow is pointing toward a hydrogen bond?

a)

4

b)

2

c)

1

d)

3

83.

Which of the following is an example of a covalent network solid?

a)

Diamond

b)

SF6

c)

CO2

d)

C2H2

84.

Once an atom has full s and p orbitals in its outermost energy level,

a)

it has a stable octet and is unreactive

b)

it is highly reactive

c)

it is slighlty reactive

d)

it can be combined easily

85.

The greater the kinetic energy of the particles in a sample of matter,

a)

the higher the temperature

b)

the lower the temperature

c)

the less heat flows away from the sample

d)

the more heat flows into the sample

86.

A molecule is a group of

a)

protons and neutrons

b)

protons and electrons

c)

covalently bonded atoms

d)

ionically bonded atoms

87.

An anion has

a)

more protons than electrons

b)

more electrons than neutrons

c)

more electrons than protons

d)

more neutrons than protons

88.

Which of the following substances has the lowest boiling point?

a)

HF

b)

Cu

c)

Cl2

d)

MgCl2

89.

the pH of a solution is 10. What is the OH- concentration?

a)

10 M

b)

4 M

c)

1 x 10-4 M

d)

1 x 10-10 M

90.

How many significant figures are in 1,000.0?

a)

1

b)

2

c)

5

d)

4

91.

Which group of teh periodic table do F and Cl belong to?

a)

actinides

b)

alkaline metals

c)

halogens

d)

chalcogens

92.

The diagram below represents which type of reaction?

a)

decomposition

b)

precipitation

c)

combustion

d)

acid/base

93.

For an exothermic reaction, the products

a)

are at a lower energy level than the products

b)

are at a higher energy level than the reactants

c)

have no energy

d)

are at the same energy level than the reactants

94.

Ethanol C2H5OH will dissolve....

a)

SF6

b)

NH3

c)

CCl4

d)

CH4

95.

Water has a high surface tension due to....

a)

strong dipole-dipole interactions

b)

weak dipole-dipole interactions

c)

strong hydrogen bond interactions

d)

weak hydrogen bond interactions

96.

How are frequency and wavelength related?

a)

they are directly proportional to each other

b)

they are indirectly proportional to each other

c)

they are not related to each other

d)

frequency and wavelength are the same

97.

Which liquid will have the lowest freezing point?

a)

0.3M Na3PO4

b)

0.6 M C6H12O6

c)

0.3 M NaCl

d)

0.9 M C12H22O11

98.

A very low value of the equilibrium constant for a reaction can indicate that...

a)

reactants are favored

b)

products are favored

c)

equilibrium is reached slowly

d)

equilibrium has been reached

99.

At high pressures, how does the volume of a real gas compare with the volume of an ideal gas under the same conditions?

a)

It depends on the gas

b)

it is less

c)

it is greater

d)

it is the same

100.

As you move from left to right across the second period of teh periodic table----

a)

atomic radius increases

b)

ionization energy increases

c)

electronegativity decreases

d)

atomic mass decreases

Similar Resources on Wayground

Ch. 20 - Nuclear Reactions

104 questions

Ch. 20 - Nuclear Reactions

quiz

Worksheet

•

8th - 12th Grade

Renewable Energy vs. Non-Renewable Energy (Fossil Fuels)

95 questions

Renewable Energy vs. Non-Renewable Energy (Fossil Fuels)

quiz

Worksheet

•

10th - 12th Grade

C02 Trends Atomic/Ionic Radii

96 questions

C02 Trends Atomic/Ionic Radii

quiz

Worksheet

•

9th - 12th Grade

Chemical Compounds Review Quizizz

100 questions

Chemical Compounds Review Quizizz

quiz

Worksheet

•

8th - 12th Grade

Unit 1 Exam Review

100 questions

Unit 1 Exam Review

quiz

Worksheet

•

7th - 10th Grade

Honors Chem Chapter 3

95 questions

Honors Chem Chapter 3

quiz

Worksheet

•

10th Grade

Ionic Bonds

99 questions

Ionic Bonds

quiz

Worksheet

•

10th Grade

Final Review

103 questions

Final Review

quiz

Worksheet

•

10th - 11th Grade