Free Printable Part 1 Chemistry I Fall Semester Exam

1.

What state of matter has a definite shape and volume?

a)

solid

b)

liquid

c)

gas

d)

plasma

2.

Which subatomic particle contributes the least to the mass of an atom?

a)

nucleon

b)

electron

c)

proton

d)

neutron

3.

The difference in mass of isotopes of the same element is because of different numbers of ______ in the nucleus.

a)

protons

b)

neutrons

c)

electrons

d)

positrons

4.

______ is an example of homogeneous matter.

a)

wood

b)

sugar

c)

concrete

d)

pizza

5.

Salt is dissolved in water. This change is _____

a)

electrolysis

b)

decomposition

c)

chemical

d)

physical

6.

Compounds can usually be broken down into their elements by:

a)

physical change

b)

distillation

c)

chemical change

d)

filtering

7.

The electron configuration for a nitrogen atom is:

a)

$1s^22s^23p^23s^1$

b)

$1s^22s^22p^3$

c)

$1s^22s^43p^1$

d)

$1s^22s^23s^3$

8.

Which of the following are located in the nucleus of an atom?

i) protons

ii) Neutrons

iii) electrons

a)

protons, neutrons, and electrons

b)

protons and neutrons only

c)

neutrons and electrons only

d)

protons and electrons only

9.

consider a neutral Na atom and a $Na^+$ ion. Which of the following is true?

a)

Both contain the same number of protons and electrons

b)

The ion contains one more proton than the neutral atom

c)

The ion contains one more electron than the neutral atom

d)

The ion contains one less electron than the neutral atom

10.

The modern periodic table is in the order of:

a)

neutron number

b)

mass number

c)

atomic number

d)

spin quantum number

11.

An element with seven valence electrons would be a:

a)

metal

(Group 3 element)

b)

metalloid

(D block element)

c)

noble gas

(group 18 element)

d)

halogen

(group 17 element)

12.

The correct formula for the compound made of $Cr^{+3}$ and $Te^{-2}$ is:

a)

CrTe

b)

$Cr_2Te_3$

c)

$Cr_3Te_2$

d)

$CrTe_3$

13.

$CaBr_2$ is correctly called

a)

calcium bromate

b)

calcium bromide

c)

calcium dibromide

d)

calcium bromite

14.

The formula for copper I chloride is:

a)

CuCl

b)

$CuCl_2$

c)

$Cu_2Cl$

d)

$CuClO_3$

15.

The formula for calcium carbonate is:

a)

CaC

b)

$Ca_2C$

c)

$Ca\left(CO_3\right)$

d)

$Ca_2\left(CO_3\right)$

16.

The formula for sodium sulfite is:

a)

$S_2\left(SO_3\right)$

b)

$S_2\left(SO_4\right)$

c)

$Na_2\left(SO_4\right)$

d)

$Na_2\left(SO_3\right)$

17.

A physical blend of two or more components

a)

mixture

b)

products

c)

vapor

d)

reactant

18.

Part of a sample having uniform composition and properties

a)

Mixture

b)

homogenous

c)

reactant

d)

vapor

19.

Not uniform in composition

a)

homogeneous

b)

heterogeneous mixture

c)

reactant

d)

product

20.

The smallest particle of an element that retains the properties of that element

a)

proton

b)

nucleus

c)

atom

d)

electron

21.

A positively charged subatomic particle

a)

Proton

b)

nucleus

c)

atom

d)

electron

22.

A negatively charged subatomic particle

a)

proton

b)

electron

c)

neutron

d)

nucleus

23.

A subatomic particle with no charge

a)

Proton

b)

Electron

c)

Neutron

d)

Nucleus

24.

The central part of an atom, containing protons and neutrons

a)

Proton

b)

Neutron

c)

Nucleus

d)

electron

25.

Amount of matter an object contains

a)

mass

b)

compound

c)

element

d)

homogeneous

26.

substance that cannot be changed into simpler substances by chemical means

a)

mass

b)

chemical reaction

c)

compound

d)

element

27.

composed of two or more substances chemically combined in a fixed proportion

a)

mass

b)

chemical reaction

c)

compound

d)

element

28.

process in which substances are changed into different substances

a)

chemical reaction

b)

element

c)

homogeneous

d)

compound

29.

Atoms with the same number of protons but different numbers of neutrons in the nucleus of the atom

a)

mass number

b)

atomic mass unit

c)

atomic number

d)

isotope

30.

the number of protons in the nucleus of an element

a)

atomic number

b)

atomic mass

c)

isotope

d)

mass number

31.

Which of the following elements is a transition metal?

a)

cesium

b)

copper

c)

tellurium

d)

aluminum

32.

What is the charge of a cation?

a)

a positive charge

b)

no charge

c)

a negative charge

d)

the charge depends on the size of the nucleus

33.

In which of the following groups of ions are the charges shown correctly?

a)

$Li^-,\ O^{-2},\ S^{+2}$

b)

$Ca^{+2},\ Al^{+3},\ Br^-$

c)

$K^{-2},\ F^-,\ Mg^{+2}$

d)

$Na^+,\ I^-,\ Rb^-$

34.

The diameter of a carbon atom is 0.000000000154 m

what is this number expressed in scientific notation?

a)

$1.54\ x\ 10^{12}\ m$

b)

$1.54\ x\ 10^{-12}\ m$

c)

$1.54\ x\ 10^{10}\ m$

d)

$1.54\ x\ 10^{-10}\ m$

35.

Which of the following measurements contain two significant figures?

a)

0.00400 L

b)

0.00404 L

c)

0.00044 L

d)

0.00440 L

36.

In which of the following is the number of neutrons correctly shown?

a)

Fluorine-19

has 0 neutrons

b)

Astatine-75

has 108 neutrons

c)

Magnesium-24

has 24 neutrons

d)

Uranium 238

has 146 neutrons

37.

of the elements Pt, V, Li, and Kr, which is a nonmental?

a)

Pt

b)

V

c)

Li

d)

Kr

38.

How many electrons does nitrogen want to gain to achieve a noble gas configuration?

a)

1

b)

2

c)

3

d)

4

39.

What type of ions have names ending in -ide?

a)

only cations

b)

only anions

c)

only metal ions

d)

only gaseous ions

40.

Which of the following compounds contain the lead II ion?

a)

$PbO$

b)

$PbCl_4$

c)

$Pb_2O$

d)

$Pb_2S$

41.

What is the correct formula for barium chloride?

a)

$Ba\left(ClO\right)_2$

b)

$Ba\left(ClO_2\right)_2$

c)

$Ba\left(ClO_3\right)_2$

d)

$BaCl_2$

42.

If you have 1 kilogram of iron and break it into smaller pieces, the density of each individual smaller piece will

a)

be smaller than the original density

b)

be more than the original density

c)

be the same as the original density because density is an intensive property

d)

impossible to know what would happen to the density of the iron

43.

Why do elements in the same group on the periodic table have similar properties?

a)

they have nearly the same mass

b)

they have similar arrangements of electrons

c)

the atoms are the same size

d)

they have the same densities

44.

What is the difference between a polyatomic ion that has -ite in its name versus one that has -ate in its name?

a)

the -ite ion will have less Oxygen while the -ate ion will have more oxygen

b)

the -ite ion will be positively charged while the -ate ion will be negative charged

c)

the -ite ion will contain iron only and the -ate ion will contain potassium

d)

the -ite ion will have more oxygen while the -ate ion will have less oxygen

45.

What atom matches this electron configuration?
1s²2s²2p⁶3s²

a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

46.

What electron configuration matches an oxygen atom?

a)

1s²2s²2p⁶3s2, 3p⁶4s²3d¹⁰4p⁵

b)

1s²2s²2p⁴

c)

1s²2s²2p⁶

d)

1s²2s²2p⁶3s²3p⁶4s²3d¹

47.

How many significant figures?

0.150

a)

1

b)

2

c)

3

d)

4

48.

Which diagram shows the MOST dense object?

a)

left

b)

center

c)

right

49.

A block of aluminum occupies a volume of 15.0 mL and weighs 45.0 g. What is its density?

a)

3 g/mL

b)

0.3333 g/mL

c)

675 g/mL

d)

I have no idea

50.

How many electrons can fit in the first energy level?

a)

8

b)

2

c)

4

d)

6

51.

Which would describe an electron that has gained energy and jumped to another shell?

a)

ground state

b)

excited state

c)

valence

d)

core

52.

Which of the following colors would be the lowest energy?

a)

red

b)

orange

c)

green

d)

violet

53.

Light is emitted when an electron moves from the ________ state to the _________ state

a)

excited, ground

b)

ground, excited

54.

The lines in the emission spectrum for hydrogen are formed from ___.

a)

energy given off when the electron moves from higher energy levels to lower energy levels

b)

electrons given off as hydrogen burns

c)

protons given off when protons move from higher energy levels to lower energy levels

d)

electrons given off as hydrogen cools

55.

When heated, electrons are ____________.

a)

annoyed

b)

irritated

c)

excited

d)

angered

56.

Cations are...

a)

Positive

b)

Negative

c)

Neutral

d)

Purring

57.

Flame tests are most useful for

a)

blood testing

b)

watching fireworks

c)

identification of elements

d)

none of the above

58.

This is a correct dot diagram for oxygen (O)

a)

true

b)

false

59.

This is a correct dot diagram for fluorine (F)

a)

true

b)

false

60.

What is the octet rule?

a)

Elements can only have 8 electrons in its outermost shell

b)

The elements must form an octopus like structure

61.

What are valence electrons?

a)

The innermost electrons

b)

The outermost electrons

62.

Label the states of matter

a)

liquid

b)

gas

c)

solid

d)

ice

1

2

3

1)

2)

3)

63.

Label the 3 states of matter shown here

a)

Solid

b)

Liquid

c)

Gas

1

2

3

1)

2)

3)

64.

Match the following properties with the state of matter

a)

Definite shape and volume

1.

Solid

b)

No defined shape, but has a definite volume

2.

Liquid

c)

No definite shape or volume

3.

Gas

65.

Match the arrangement to the state of matter

a)

1.

Solid

b)

2.

Gas

c)

3.

Liquid

d)

4.

Plasma

Part 1 Chemistry I Fall Semester Exam

Total questions: 65

Worksheet time: 42mins

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