Free Printable Midterm Review

1.

Place these metric units in order from smallest to largest: kilometer, millimeter, meter, centimeter.

a)

millimeter, centimeter, meter, kilometer

b)

centimeter, millimeter, meter, kilometer

c)

meter, centimeter, millimeter, kilometer

d)

kilometer, meter, centimeter, millimeter

2.

If a neutral atom of aluminum has 13 protons and 15 neutrons, what is its mass number?

a)

26

b)

27

c)

28

d)

29

3.

How many atoms would be in 1.00 mol of arsenic?

a)

$6.022\times10^{22}$

b)

$6.022\times10^{23}$

c)

$6.022\times10^{24}$

d)

$6.022\times10^{25}$

4.

Which set correctly lists metric base units for the following measurements: length, volume, mass, time, and temperature?

a)

meter, liter, kilogram, second, kelvin

b)

meter, milliliter, gram, minute, Celsius

c)

centimeter, liter, gram, second, kelvin

d)

meter, liter, gram, hour, Celsius

5.

Organic chemistry focuses on which of the following?

a)

Reactions of ionic compounds in water

b)

Compounds that contain carbon

c)

Measuring reaction rates only

d)

Structure of atomic nuclei

6.

Analytical chemistry is best described as the study of what?

a)

Energy changes in reactions only

b)

Identification and composition of materials

c)

Behavior of gases at high pressure

d)

Motion of celestial bodies

7.

Biochemistry primarily studies what?

a)

Processes in living things

b)

Bonding in metals

c)

Crystal structures of salts

d)

Radioactive decay series

8.

Which element would be a good substitute for sulfur because it is in the same group and has similar properties?

a)

Oxygen

b)

Chlorine

c)

Sodium

d)

Argon

9.

Write $0.000000764$ in scientific notation.

a)

$7.64\times10^{-6}$

b)

$7.64\times10^{-7}$

c)

$7.64\times10^{-8}$

d)

$7.64\times10^{7}$

10.

According to VSEPR theory, what is the shape of an $AB_3$ molecule?

a)

Linear

b)

Trigonal planar

c)

Tetrahedral

d)

Bent

11.

What does VSEPR theory describe?

a)

Electrons pair to attract each other strongly

b)

Electron pairs arrange themselves to be as far apart as possible

c)

Only the shapes of ionic compounds

d)

Only the energies of electrons in atoms

12.

What is the most electronegative element on the periodic table?

a)

Oxygen

b)

Chlorine

c)

Fluorine

d)

Nitrogen

13.

What happens to atomic radius as you move from left to right across a period on the periodic table?

a)

It increases steadily

b)

It decreases

c)

It remains exactly constant

d)

It first increases then decreases

14.

Which blocks make up the main-group elements on the periodic table?

a)

s and d blocks

b)

p and d blocks

c)

s and p blocks

d)

f and d blocks

15.

Which groups are very reactive on the periodic table?

a)

Groups 3 and 12

b)

Groups 1, 2, and 17

c)

Groups 8 and 18

d)

Groups 14 and 15

16.

Which group is very unreactive on the periodic table?

a)

Group 1

b)

Group 2

c)

Group 17

d)

Group 18

17.

What does the periodic law state?

a)

Properties of elements repeat with their atomic masses

b)

Physical and chemical properties of elements are periodic functions of their atomic numbers

c)

Nuclei of elements determine their color

d)

Valence electrons are the same within a period

18.

Why are alkali metals and alkaline earth metals rarely found alone in nature?

a)

They are too reactive and form compounds readily

b)

They are too heavy to occur naturally

c)

They are gases at room temperature

d)

They have no valence electrons

19.

What do we call the elements in groups 3–12?

a)

Metalloids

b)

Transition metals

c)

Halogens

d)

Noble gases

20.

What do we call the elements in group 17?

a)

Alkali metals

b)

Transition metals

c)

Halogens

d)

Noble gases

21.

What is the noble gas electron configuration for calcium ( $\mathrm{Ca}$ )?

a)

$[\mathrm{Ne}]3s^2$

b)

$[\mathrm{Ar}]4s^2$

c)

$[\mathrm{Kr}]5s^2$

d)

$[\mathrm{Ar}]3d^2$

22.

What did Mendeleev observe about elements to create the first periodic table?

a)

Their average densities

b)

Their properties and how they repeat

c)

Their boiling points only

d)

Their isotopic abundances

23.

Which electrons are involved in bonding?

a)

Core electrons

b)

Valence electrons

c)

All electrons equally

d)

Only d-electrons

24.

Identify the element in group 2, period 5.

a)

Calcium (Ca)

b)

Barium (Ba)

c)

Strontium (Sr)

d)

Magnesium (Mg)

25.

How many valence electrons does an element have if its electron configuration ends with $2p^4$ ?

a)

4

b)

5

c)

6

d)

8

26.

To which block of elements does zinc belong?

a)

s block

b)

p block

c)

d block (transition metals)

d)

f block

27.

Molar mass is the numerical equivalent of what periodic table value (but expressed in $\mathrm{gmol^{ }}$ instead of amu)?

a)

Atomic number

b)

Atomic mass

c)

Electronegativity

d)

Ionization energy

28.

Rutherford’s gold foil experiment showed the presence of what in the center of an atom?

a)

Electron cloud

b)

Nucleus

c)

Proton shell

d)

Neutron ring

29.

Rutherford’s experiment also showed that an atom is mostly what?

a)

Solid matter

b)

Empty space

c)

Uniform positive charge

d)

Dense electrons

30.

What is the charge of a proton?

a)

Negative

b)

Positive

c)

Neutral

d)

Varies by element

31.

What is the charge of an electron?

a)

Positive

b)

Neutral

c)

Negative

d)

Depends on the atom

32.

What is the charge of a neutron?

a)

Negative

b)

Neutral

c)

Positive

d)

Depends on isotopes

33.

The word atom comes from a Greek word meaning what?

a)

Visible

b)

Indivisible

c)

Electrified

d)

Tiny

34.

Which law states that matter can neither be created nor destroyed?

a)

Law of Definite Proportions

b)

Law of Multiple Proportions

c)

Law of Conservation of Mass

d)

Boyle’s Law

35.

Which subatomic particle is equal in number to the atomic number of an element?

a)

Neutrons

b)

Protons

c)

Electrons

d)

All subatomic particles

36.

What was learned from Thomson’s cathode ray tube experiment?

a)

Atoms are indivisible

b)

Electrons are small particles with negative charge and measurable mass

c)

Protons are negatively charged

d)

Neutrons orbit the nucleus

37.

If the isotope symbol is written $^{29}_{13}\mathrm{Al}$ , how many neutrons does the atom have?

a)

13

b)

15

c)

16

d)

29

38.

Which is the correct nuclear symbol for carbon-14?

a)

$^{14}_{6}\mathrm{C}$

b)

$^{6}_{14}\mathrm{C}$

c)

$^{14}\mathrm{C}_6$

d)

$^{12}_{6}\mathrm{C}$

39.

What is the mass number of P-35?

a)

15

b)

30

c)

31

d)

35

40.

Which is the complete ground-state electron configuration for sulfur ( $\mathrm{S}$ )?

a)

$1s^2\,2s^2\,2p^6\,3s^2\,3p^4$

b)

$1s^2\,2s^2\,2p^6\,3s^2\,3p^6$

c)

$[\mathrm{Ne}]3s^2\,3p^6$

d)

$[\mathrm{Ar}]4s^2$

41.

Are changes of state like evaporation, condensation, and melting physical or chemical changes?

a)

Chemical

b)

Physical

c)

Both chemical and physical

d)

Neither

42.

Would trail mix or Chex Mix be considered a heterogeneous or homogeneous mixture?

a)

Homogeneous mixture

b)

Heterogeneous mixture

43.

If you divide $5.78$ by $3.2$ , how many significant figures should the final answer have?

a)

1

b)

2

c)

3

d)

4

44.

Round 14.006 to 3 sig figs

a)

14

b)

14.01

c)

14.0

d)

14.01

45.

How many significant figures are in the measurement $4.005$ ?

a)

2

b)

3

c)

4

d)

5

46.

Which equation correctly expresses density?

a)

density = volume/mass

b)

density = mass/volume

c)

density = mass × volume

d)

density = mass − volume

47.

The right side of the periodic table is made up primarily of which type of elements?

a)

Metals

b)

Nonmetals

c)

Metalloids

d)

Transition metals

48.

What are the rows on the periodic table called?

a)

Groups

b)

Periods

c)

Families

d)

Series

49.

What are the columns on the periodic table called?

a)

Periods

b)

Groups

c)

Rows

d)

Blocks

50.

Homogeneous mixtures are also commonly called what?

a)

Colloids

b)

Suspensions

c)

Solutions

d)

Alloys only

51.

If a substance has a formula like HCl, is it a mixture, an element, or a compound?

a)

Mixture

b)

Element

c)

Compound

d)

Solution

52.

What is a nanometer?

a)

$1\times10^{-6}$ meter

b)

$1\times10^{-9}$ meter

c)

$1\times10^{-12}$ meter

d)

$1\times10^{9}$ meters

53.

What is a picometer?

a)

$1\times10^{-6}$ meter

b)

$1\times10^{-9}$ meter

c)

$1\times10^{-12}$ meter

d)

$1\times10^{-15}$ meter

54.

When dividing numbers in scientific notation, what do you do with the exponents?

a)

Add them

b)

Subtract the denominator exponent from the numerator exponent

c)

Multiply them

d)

Ignore them

55.

Calculate the mass of $4.3$ moles of phosphorus ( $\mathrm{P}$ ). Choose the best rounded answer for two significant figures.

a)

$120\,\mathrm{g}$

b)

$130\,\mathrm{g}$

c)

$133.17\,\mathrm{g}$

d)

$140\,\mathrm{g}$

56.

What did Thomson and Rutherford disprove about Dalton’s atomic theory?

a)

Atoms are indivisible and cannot be broken down

b)

Atoms have dense positive nuclei

c)

All matter is made of elements

d)

Mass is conserved in reactions

57.

In Rutherford’s gold foil experiment, some alpha particles were deflected sharply or bounced back. What did this reveal must be in the atom?

a)

A diffuse negative cloud

b)

A central region of positive charge (nucleus)

c)

Only empty space

d)

Only neutrons in the center

Midterm Review –

Total questions: 57

Worksheet time: 29mins

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