Free Printable General Chemistry Concepts

1.

Choose the 3 fundamental sub atomic particle of matter.

a)

photon

b)

proton

c)

nucleus

d)

neutron

e)

electron

2.

What do you call this famous experiment that leads to the discovery of the nucleus of the atom?

a)

Millikan Experiment

b)

Alpha bombardment experiment

c)

Gold foil experiment

d)

All of the above

3.

Subatomic particles found in the nucleus of an atom

a)

proton

b)

photon

c)

electron

d)

neutron

e)

meson

4.

Number of moles of sugar in 547.2 gram are:

(Mol. mass of sugar = 342 g/mole)

a)

1.6

b)

2.2

c)

342

d)

548

5.

Which statement best describes an element?

a)

any combination of two or more atoms of different types

b)

a pure substance made up of only one kind of atom

c)

a substance containing only carbon atoms

d)

any kind of crystal

6.

Which of the following changes is a physical change of matter?

a)

water evaporating

b)

paper burning

c)

a nail rusting

d)

a silver spoon tarnishing

7.

Which of the following changes is a chemical change of matter?

a)

ice melting to produce water

b)

vinegar combining with baking soda to produce carbon dioxide

c)

water boiling to produce water vapor

d)

liquid silica solidifying to form glass

8.

The horizontal rows of the periodic table are called

a)

periods

b)

columns

c)

groups

d)

families

9.

The SI base units for time and temperature are

a)

hour and degree Celsius.

b)

second and degree Celsius.

c)

hour and kelvin.

d)

second and kelvin.

10.

The number of significant figures in the measurement 170.040 km is

a)

Three

b)

Four

c)

Five

d)

Six

11.

Expressed in scientific notation, 0.0930 m is

a)

93 X 10^-3 m

b)

9.3 X 10^-3 m.

c)

9.30 X 10^-2 m.

d)

9.30 X 10^-4 m.

12.

Atoms of the same element that have a different number of neutrons are called

a)

ions

b)

isotope

c)

isomer

d)

radioactive

13.

Atoms that gain or lose electrons become

a)

ions

b)

isotopes

c)

isopmers

d)

radioactive

14.

What type of bond is formed between atoms that share their valence electrons?

a)

Hydrogen bond

b)

James bond

c)

Covalent bond

d)

Ionic bond

15.

What is the atomic number?

a)

the number of protons

b)

the number of protons and neutrons

c)

the number of neutrons

d)

the number of protons and electrons

16.

What is the mass number defined as?

a)

the number of protons

b)

the number of protons and neutrons

c)

the number of neutrons

d)

the number of protons and electrons

17.

An electron occupies the lowest energy orbital that can receive it.

a)

Hund’s rule

b)

Pauli exclusion principle

c)

Bohr model of the atom

d)

Aufbau principle

18.

Is chicken noodle soup a Homogeneous or Heterogeneous mixture?

a)

Homogeneous

b)

Heterogeneous

c)

Neither

d)

Both

19.

Chemical Formulas ...

a)

are written in alphabetical order

b)

represent the destruction or creation of atoms

c)

represent how atoms are arranged in a chemical reaction

20.

The compounds or elements present at the end of a reaction

a)

reactants

b)

catalyst

c)

products

d)

energy

21.

The compounds and elements that are present at the beginning of a reaction:

a)

reactants

b)

catalyst

c)

products

d)

energy

22.

Which of the following reactions is a combustion reaction ?

a)

MgCO3 + O2 → MgO + CO2

b)

C3H8 + 5O2 → 3CO2 + 4H2O

c)

6CO2 + 6H2O → C6H12O6 + 6O2

d)

6CO2 + 6H2O → C6H12O6 + 6O2

23.

What is the law of Conservation of Mass?

a)

A measure of how much mass is created or destroyed.

b)

Mass can neither be created nor destroyed during a chemical reaction.

24.

Which of the following is a decomposition reaction?

a)

MgCo3 --> MgO + CO2

b)

SO3 + H2O --> H2SO4

c)

2 Mg + O2 --> 2MgO

25.

An atom of carbon has 6 protons and 7 neutrons in its nucleus. If the atom is neutral, how many electrons does it have?

a)

0

b)

7

c)

6

d)

13

26.

A substance with a pH of 8 is a

a)

acid

b)

base

c)

neutral

27.

The electrons in the outermost energy level are called

a)

valence

b)

ions

c)

covalent

d)

farthest out

28.

Which of the following would be considered most acidic?

a)

1

b)

3

c)

7

d)

13

29.

The image shows the periodic grid for SODIUM. What is Sodium's atomic mass?

a)

11

b)

12

c)

23

d)

Impossible to tell

30.

Which of the following is described as the basic unit of matter?

a)

Element

b)

Atom

c)

Molecule

d)

Compound

31.

These particles are found in the nucleus of the atom.

a)

protons only

b)

protons and electrons

c)

electrons only

d)

protons and neutrons

32.

The mass number is the total of the protons plus the neutrons in the atom.

a)

True

b)

False

33.

Which subatomic particle has a negative charge?

a)

proton

b)

electron

c)

neutron

d)

quark

34.

How many neutrons would you expect the average gold atom to have given the information shown?

a)

79

b)

118

c)

197

d)

276

35.

Who is the person credited with the formation of the "plum pudding" model?

a)

Thomson

b)

Rutherford

c)

Bohr

d)

Dalton

36.

What subatomic particle represents the "plums" in the "plum pudding" model?

a)

neutrons

b)

protons

c)

electrons

37.

Chadwick is credited with discovering which part of the atom?

a)

nucleus

b)

protons

c)

electrons

d)

neutrons

38.

Who is credited with developing model D?

a)

Thomson

b)

Dalton

c)

Bohr

d)

Rutherford

39.

Who discovered the subatomic particle "electron"?

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

40.

Who established that "electrons move around the nucleus at fixed distances called orbitals"?

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

41.

What is the meaning of the greek word "atomos"?

a)

Invencible

b)

Invisible

c)

Indivisible

d)

Independent

42.

What electron configuration matches an oxygen atom?

a)

1s²2s²2p⁶3s2, 3p⁶4s²3d¹⁰4p⁵

b)

1s²2s²2p⁴

c)

1s²2s²2p⁶

d)

1s²2s²2p⁶3s²3p⁶4s²3d¹

43.

The electron configuration of an atom is 1s²2s²2p⁶. The number of electrons in the atom is

a)

3

b)

6

c)

8

d)

10

44.

What is this element?
1s²2s²2p⁶3s²

a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

45.

There are 4 different types of subshells s,p,d,f

a)

true

b)

false

46.

Identify the Electron Configuration for Aluminum (Al)

a)

1s²2s²2p⁶3s²3p¹

b)

1s²2s²2p⁶3s²3p³

c)

1s²2s²2p⁶3s²4p¹

47.

The chemical bond formed when two atoms share electrons is call a(n)

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

electron bond

48.

Which of the following is the reason why atoms of sodium and chlorine attract each other in a salt crystal?

a)

Sodium has a positive charge and chlorine has a negative charge

b)

Sodium has a negative charge and chlorine has a positive charge

c)

Both have a positive charge

d)

Both have a negative charge

49.

What type of bond is formed by the transfer of electrons as illustrated in this diagram?

a)

Non-polar covalent

b)

Metallic

c)

Ionic

d)

Polar covalent

50.

What do we call a covalent bond where electrons are shared UNEVENLY or UNEQUALLY?

a)

Ionic

b)

Polar Covalent

c)

Nonpolar Covalent

d)

Metallic

51.

What type of bond is shown in this image?

a)

Ionic

b)

Polar Covalent

c)

Nonpolar Covalent

d)

Metallic

52.

The chemical bond formed when two atoms share electrons is call a(n)

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

electron bond

53.

What kind of chemical bond forms between a metal and a nonmetal?

a)

ionic

b)

covalent

c)

fake

d)

metallic

54.

What is the name for an ion with a positive charge?

a)

cation

b)

anion

c)

onion

d)

union

55.

What kind of bond forms between two nonmetals?

a)

ionic

b)

covalent

c)

metallic

d)

fake

56.

Which of the following are isotopes?

a) ¹⁴₇X b) ¹⁴₆X c) ¹⁵₇X d) ¹⁵₈X

a)

a) and b)

b)

a) and c)

c)

c) and d)

d)

a) and d)

57.

How is carbon-12 different from carbon-14?

a)

They have a different number of protons

b)

they have a different number of electrons

c)

they have a different number of neutrons

58.

What do these isotopes of carbon all have in common?

a)

neutrons & mass number

b)

atomic number and neutrons

c)

atomic number and electrons

d)

protons, atomic number, and mass number

59.

In the following pair, are they isotopes or different elements.

Element x has 6 protons and 7 neutrons.

Element y has 7 protons and 7 neutrons.

a)

isotopes of same element

b)

different elements

60.

In the following pair, are they isotopes or different elements.

Element x has 27 protons and 82 neutrons.

Element y has 27 protons and 83 neutrons.

a)

isotopes of same element

b)

different elements

61.

What subatomic particle changes in an ion?

a)

The number of electrons

b)

The number of protons

c)

The number of neutrons

62.

What charge does an atom have when it GAINS electrons?

a)

Positive

b)

Negative

c)

Neutral

63.

How many protons and electrons are present: $Cl^-$

a)

Protons: 17

Electrons: 18

b)

Protons: 17

Electrons: 1

c)

Protons: 18

Electrons: 17

d)

Protons: 1

Electrons: 17

64.

How many protons and electrons are present: $As^{3+}$

a)

Protons: 30

Electrons: 33

b)

Protons: 3

Electrons: 0

c)

Protons: 33

Electrons: 30

d)

Protons: 3

Electrons: 33

65.

The atom with the largest atomic radius in Group 18 is -

a)

Ar

b)

He

c)

Kr

d)

Rn

66.

As you move down a group, atomic radius increases because -

a)

you add more and more neutrons

b)

you add more and more protons

c)

you add more and more shells (energy levels)

d)

you add more atomic mass

67.

Francium (Fr) has the lowest ionization energy in Group 1 because -

a)

it has the smallest number of valence electrons

b)

it has the greatest atomic mass

c)

it has the greatest number of protons, so it attracts its electrons the strongest

d)

its 1 valence electron is very far from the nucleus, so little energy is needed to remove it

68.

The element with the smallest ionization energy in Period 6 is -

a)

Rn

b)

Cs

c)

Os

d)

Tm

69.

Which of the following will have a higher electronegativity than arsenic (As)?

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

70.

What is the amount of energy required to remove an electron from an atom?

a)

atomic energy

b)

ionization energy

c)

ionic energy

d)

electron energy

71.

What is a measure of the tendency of an atom to attract a bonding pair of electrons when the atom is in a compound?

a)

ionization energy

b)

electropositivity

c)

electronegativity

d)

electron energy

72.

What reaction has the following general formula:

A + CD --> C + AD

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

73.

What reaction has the following general formula:
$C_xH_y\ +\ O_2\ ->CO_{2\ }+\ H_2O$

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

74.

What is the general reaction scheme for a single replacement reaction?

a)

A + B --> AB

b)

AB --> A + B

c)

A + CD --> C + AD

d)

AB + CD --> CB + AD

e)

$C_xH_y+O_2\ ->\ CO_2+H_2O$

75.

What is the general reaction scheme for a combination reaction?

a)

A + B --> AB

b)

AB --> A + B

c)

A + CD --> C + AD

d)

AB + CD --> CB + AD

e)

$C_xH_y+O_2\ ->\ CO_2+H_2O$

76.

What is the general reaction scheme for a double replacement reaction?

a)

A + B --> AB

b)

AB --> A + B

c)

A + CD --> C + AD

d)

AB + CD --> CB + AD

e)

$C_xH_y+O_2\ ->\ CO_2+H_2O$

77.

What reaction has the following general formula:

AB --> A + B

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

78.

What reaction has the following general formula:

A + B --> AB

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

79.

What is the mole ratio of H2O to H3PO4 in the following chemical equation?

$P_4O_{10}+6H_2O\ \rightarrow\ 4H_3PO_4$

a)

1 to 6

b)

3 to 2

c)

4 to 6

d)

2 to 3

80.

In the equation $Al_2\left(SO_4\right)3+3Ca\left(OH\right)_2\ \rightarrow\ 3CaSO_4\ +2Al\left(OH\right)_3$ , , the mole ratio of calcium hydroxide to aluminum hydroxide is:

a)

1 : 3

b)

2 : 3

c)

1 : 1

d)

3 : 2

81.

For the reaction represented by the equation $N_2+3H_{2\ }\rightarrow\ 2NH_3$ , how many moles of nitrogen (N2) are required to produce 18 grams of ammonia (NH3)?

a)

0.9 mol

b)

18 grams

c)

0.53 mol

d)

36 grams

82.

For the reaction represented by the equation $Pb\left(NO_3\right)_2+2KI\ \rightarrow\ PbI_2+2KNO_3$ how many moles of lead iodide $\left(PbI_2\right)$ are produced of 300 grams potassium iodide $\left(KI\right)$ when $Pb\left(NO_3\right)_2$ is in excess?

a)

114.78 mol PbI₂

b)

0.904 grams PbI₂

c)

0.904 mol PbI₂

d)

114.78 grams PbI₂

83.

Which expression can be used to solve a mass-to-mole conversion for the equation HCL -----> H₂ + Cl₂? Given: Mass of HCl and unknown: Mol of Cl2

a)

$mass\ HCl\ x\ \frac{1\ mol\ HCl}{molar\ mass\ HCl}\ x\ \frac{1\ mol\ Cl2}{2\ mol\ HCl}$

b)

$mass\ HCl\ x\frac{1\ mol\ Cl2\ }{2\ mol\ HCl}$

84.

Balance this reaction: ____ RbNO₃ + ____ BeF₂ ----> ____ Be(NO₃)₂ + ____ RbF

a)

1,1,1,1

b)

1,2,1,1

c)

2,1,1,2

d)

2,1,2,1

85.

___KNO₃ → ___KNO₂ + ___O₂

What coefficients are needed to balance the reaction?

a)

2, 2, 1

b)

2, 3, 2

c)

1, 2, 2

d)

1, 3, 1

86.

What is one assumption that must be made for the kinetic molecular theory to be applied to gases?

a)

Collisions between gas particles are inelastic.

b)

Gases consist of closely spaced particles.

c)

Gas particles move in constant straight line motion.

d)

Each gas particle has a definite volume.

87.

The pressure exerted by a gas does not depend on

a)

temperature.

b)

volume.

c)

number of moles present.

d)

the identity of the gas.

88.

Of these three states of matter, which one has the most kinetic energy?

a)

Solid

b)

Liquid

c)

Gas

89.

Under what temperature and pressure conditions does a gas behave the most like and ideal gas? (Choose all that apply.)

a)

high pressure (above 1 atm)

b)

low temperature (below 273 K)

c)

standard temperature

(273 K)

d)

standard pressure (1 atm)

90.

What is one assumption that must be made for the kinetic molecular theory to be applied to gases?

a)

Collisions between gas particles are elastic.

b)

Gases consist of closely spaced particles.

c)

Gas particles rarely move.

d)

Each gas particle has a definite volume.

91.

According to Charle's Law, volume and temperature are directly related. Explain what is meant by stating that volume and temperature are directly related. $\frac{V_1}{T_1}\ =\ \frac{V_2}{T_2}$

a)

Volume increases, temperature decreases.

b)

Volume increases, temperature increases.

c)

Volume decreases, temperature increases.

d)

Temperature increases, volume decreases.

92.

What units must temperature always be in for ALL the gas laws?

a)

Celcius

b)

Kelvin

c)

Fahrenheit

d)

Kelvin or Celcius

93.

Pressure is caused by:

a)

Gas molecules colliding with surfaces

b)

Gas molecules reacting with each other

c)

Gas molecules colliding with each other

d)

Gravity

94.

The table shows the pH of several solutions. Which solution is the most acidic?

a)

vinegar

b)

milk

c)

water

d)

bleach

95.

Four substances were tested for pH, lemon juice (pH 2), baking soda (pH 9), bleach (pH 12), and milk (pH 6). Which of the following correctly lists the substances from most basic to acidic?

a)

lemon juice, milk, baking soda, bleach

b)

bleach, baking soda, milk, lemon juice

c)

milk, lemon juice, baking soda, bleach

d)

baking soda, bleach, lemon juice, milk

96.

Phenolphthalein is pink in an aqueous solution having a pH of

a)

2

b)

7

c)

5

d)

12

97.

$H_2CO_3$

a)

Strong Acid

b)

Weak Acid

c)

Strong Base

d)

Weak Base

98.

NaOH

a)

Strong Acid

b)

Weak Acid

c)

Strong Base

d)

Weak Base

99.

The pH scale is used to know what?

a)

Your temperature

b)

Know one knows

c)

The colors of acids and bases

d)

The strength of acids and bases

100.

Acids have a pH of _______________.

a)

below 7

b)

above 7

c)

exactly 7

General Chemistry Concepts

Total questions: 100

Worksheet time: 1hrs 5mins

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