Free Printable Chemistry Study Quiz

1.

Metals are

a)

Good conductors, malleable, ductile, lusterous

b)

Poor conductors, malleable, brittle, lusterous

c)

Good conductors, brittle, ductile, lusterous

d)

Poor conductors, malleable, ductile, dull

2.

Nonmetals are

a)

Poor conductors

b)

Good conductors

c)

Semi-conductors

3.

Metalloids are

a)

Semi-conductors, have some characteristics of both metals and nonmetals

b)

Good conductors, have some characteristics of both metals and nonmetals

c)

Poor conductors, have some characteristics of both metals and nonmetals

d)

Semi-conductors, have none of the characteristics of both metals and nonmetals

4.

Noble gases are

a)

Unreactive

b)

Highly reactive

c)

Have no atoms

d)

Slightly reactive

5.

Solutions are mixtures that are

a)

Always made with water

b)

Homogeneous

c)

Heterogeneous

d)

Always made with salt

6.

Extensive Property Examples

a)

Mass

b)

Temperature

c)

Volume

d)

Amount of energy in a substance

e)

Melting Point

7.

Intensive Property Examples

a)

Density

b)

Melting point

c)

Temperature

d)

Boiling point

e)

Ability to conduct electricity

8.

Matter is

a)

Anything that has density and takes up space

b)

Anything that has mass and takes up space

c)

Anything that has matter and takes up space

d)

Anything that has mass and can be mapped out on scatter plots

9.

Select all of which are part of Dalton's Atomic Theory

a)

Atoms combine in small, whole-number ratios.

b)

All matter is composed of extremely small particles called atoms.

c)

Atoms of the same element are the same, atoms of different elements are different.

d)

Atoms cannot be created, subdivided, or destroyed.

e)

In chemical reactions, atoms can combine, separate, or be rearranged,

10.

An atom is

a)

The smallest part of an element that retains the chemical properties of that element

b)

The largest part of an element that retains the chemical properties of that element

c)

The smallest part of an element that retains the physical properties of that element

d)

The largest part of an element that retains the physical properties of that element

11.

What were Rutherford's conclusions in the gold foil experiment?

a)

The volume of the atom's nucleus is relatively small compared to the total volume of the atom itself.

b)

Atoms are mostly made up of empty space.

c)

Atoms are mostly made up of electrons.

d)

An atom has a densely packed bundle of matter with a positive electric charge in its center.

12.

Atomic number

a)

Number of atoms each atom of an element has

b)

Number of protons each atom of an element has

c)

Number of neutrons each atom of an element has

d)

Number of electrons each atom of an element has

13.

Which is example shows two isotopes?

a)

O

Ni

b)

O

Oxygen-20

c)

Oxygen-18

Oxygen-20

d)

C

14

14.

What are the three types of hydrogen?

a)

quiterium

b)

deuterium

c)

protium

d)

tritium

15.

Mass number

a)

Total number of neutrons and neutrons that make up an isotope's nucleus

b)

Total number of protons and neutrons that make up an isotope's nucleus

c)

Total number of protons and electrons that make up an isotope's nucleus

d)

Total number of electrons and neutrons that make up an isotope's nucleus

16.

One atomic mass unit equals

a)

1/12 the mass of a carbon-12 atom

b)

1/2 the mass of a carbon-12 atom

c)

1/8 the mass of a oxygen-8 atom

d)

1/12 the mass of a nitrogen-12 atom

17.

What is a mole?

a)

The amount of a substance that contains as many particles as there are atoms in exactly 12 grams of carbon-14

b)

The amount of a substance that contains as many particles as there are atoms in exactly 12 grams of carbon-12

c)

The amount of a substance that contains as many particles as there are atoms in exactly 14 grams of nitrogen-14

d)

The amount of a substance that contains as many particles as there are atoms in exactly 8 grams of oxygen-8

18.

Avogadro's Number

a)

6.02x10^26

b)

6.02x10^23

c)

6.02x10^22

d)

6.02x10^24

19.

In this equation, the wavelength is inversely proportional to the frequency.

$\lambda v=c$

a)

False

b)

True

20.

Photoelectric Effect

a)

The emission of electrons from a metalloid when light shines on the metalloid

b)

The emission of electrons from a nonmetal when light shines on the nonmetal

c)

The emission of electrons from a metal when light shines on the nonmetal

d)

The emission of electrons from a metal when light shines on the metal

21.

Planck's Constant

a)

$6.626x10^{-32}J\cdot s$

b)

$6.626x10^{^-34}J\cdot s$

c)

$^{6.626x10^{-33}}J\cdot s$

d)

$6.266x10^{-34}J\cdot s$

22.

E=hv

a)

Equation for speed of light

b)

Equation for energy

c)

Equation for electrons

d)

Equation for frequency

23.

For electrons to move from lower energy states to higher energy states, energy needs to be added to the atom.

a)

True

b)

Partially true

c)

False

24.

Quantum Numbers

a)

Specify the properties of atomic orbitals and the properties of protons in orbitals

b)

Specify the properties of atomic orbitals and the properties of electrons in orbitals

c)

Specify the properties of atomic orbitals and the properties of neutrons in orbitals

d)

Specify the properties of electronic orbitals and the properties of electrons in orbitals

25.

Main energy level occupied by the electron

a)

Spin Quantum Number

b)

Angular Momentum Quantum Number

c)

Principal Quantum Number

d)

Magnetic Quantum Number

26.

Shape of the orbital

a)

Magnetic Quantum Number

b)

Principal Quantum Number

c)

Angular Momentum Quantum Number

d)

Spin Quantum Number

27.

Orientation of an orbital around the nucleus

a)

Spin Quantum Number

b)

Angular Momentum Quantum Number

c)

Principal Quantum Number

d)

Magnetic Quantum Number

28.

The two fundamental spin states of an electron in an orbital (+1/2, -1/2)

a)

Principal Quantum Number

b)

Spin Quantum Number

c)

Angular Momentum Quantum Number

d)

Magnetic Quantum Number

29.

Published first periodic table

a)

Moseley

b)

Mendel

c)

Cannizaro

d)

Mendeleev

30.

The physical and chemical properties of the elements are periodic functions of their atomic numbers

a)

Periodic law

b)

Periodic constancy

c)

Intensive properties

d)

Law of conversation of properties

31.

One-half the distance between the nuclei of identical atoms that are bonded together

a)

Catonic radius

b)

Anionic radius

c)

Atomic radius

d)

Ionic radius

32.

Ionization energy-the energy required to remove an electron from a neutral atom of an element

a)

$A+energy\rightarrow A^+-e^-$

b)

$A+energy\rightarrow A^++e^-$

33.

Equation(s) for Electron Affinity

a)

$A+e^-\rightarrow A^++energy$

b)

$A+e^-\rightarrow A^-+energy$

c)

$A+e^-+energy\rightarrow A^-$

d)

$A-e^-\rightarrow A^-+energy$

34.

Covalent bonding

a)

Sharing nothing between two atoms

b)

Sharing ions between two atoms

c)

Sharing electron pairs between two atoms

d)

Sharing protons between two atoms

35.

What type of bond is this?

2.2-0.8=?

a)

ionic

b)

polar-covalent

c)

nonpolar-covalent

d)

covalent

36.

What kind of bond is this?

3.0-0.7=?

a)

Covalent

b)

Ionic

c)

Polar-covalent

d)

Nonpolar-covalent

37.

What kind of bond is this?

2.5-2.5=?

a)

covalent

b)

nonpolar-covalent

c)

polar-covalent

d)

ionic

38.

H=F

What bond is shown?

a)

Double

b)

Triple

c)

Single

39.

Resonance Structure

a)

Created when a single Lewis structure cannot correctly represent the bonding between molecules or covalent bonds

b)

Created when a single Lewis structure cannot correctly represent the bonding between molecules or ions

c)

Created when a single Lewis structure cannot correctly represent the bonding between cations or ions

d)

Created when a single Lewis structure cannot correctly represent the bonding between molecules or anions

40.

The energy released when one mole of an ionic crystalline compound is formed from gaseous ions

a)

Valence energy

b)

Ionization energy

c)

Lattice energy

d)

Bond energy

41.

Metallic bonding

a)

Forms a Sea of Energy

b)

Forms a Sea of Electrons

c)

Forms a Sea of Valences

d)

Forms a Sea of Protons

42.

Which of these is an example of a hybrid orbital?

a)

sd^2

b)

pf^7

c)

sp^3

d)

sd^5

43.

London Dispersion Forces

a)

The intermolecular force in which a hydrogen atom bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule

b)

Equal but opposite charges that are separated by a short distance

c)

The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles

d)

The forces of attraction between polar molecules

44.

Aluminum

a)

Al3-

b)

Al3+

c)

Al

d)

Ag+

45.

HF

a)

Fluoride

b)

Hydrogen fluoride

c)

Fluoric Acid

d)

Hydrofluoric acid

46.

What is the oxidation number of cesium in this compound?

CsBr

a)

6+

b)

1+

c)

1-

d)

2+

47.

What is the name of this compound?

NO

a)

Nitrogen Oxygen

b)

Nitrogen Monoxide

c)

Nitrogen Oxide

d)

Nitrogen Trioxide

48.

$H_2+Br_2\rightarrow?$

a)

$H_2Br_2$

b)

2HBr

c)

HBr

d)

$H_2Br$

49.

Atomic radii trend

a)

Increase from left to right, and decreases from top to bottom

b)

Increase from left to right, and increases from top to bottom

c)

Increase from right to left, and increases from top to bottom

d)

Increase from right to left, and decreases from top to bottom

50.

$SrO+H_2O\rightarrow?$

a)

$SrH_2O$

b)

$Sr\left(OH\right)_2$

c)

$Sr\left(OH\right)_3$

d)

$SrO_3+H_2$

Chemistry Study Quiz

Total questions: 50

Worksheet time: 27mins

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