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Honors Chemistry Midterm 2025

Total questions: 80

Worksheet time: 2hrs 45mins

Name
Class
Date
1.
What was the name of J.J Thomsons' model of atomic structure. 
a)
Electron Cloud Model 
b)
Electron Sea Model
c)
Plum Pudding Model 
d)
Bohr Model
2.
In the Thomson Model, he discovered the existence of what particle?
a)
Electrons
b)
Protons
c)
Neutrons
d)
Quarks
3.

Who concluded that electrons orbit the nucleus in specific shells?

a)

John Dalton

b)

Rutherford

c)

Thompson

d)

Bohr

4.

According to Democritus' atomic theory, atoms are _________.

a)

indivisible and indestructible

b)

composed of protons, neutrons, and electrons

c)

arranged in a plum pudding structure

d)

located in the nucleus

5.

This model was the first to show a nucleus, consisting of protons and neutron.  Electrons surround the nucleus but are not shown in distinct energy levels. 

a)

Democritus's model of the atom

b)

The "Rutherford Model" of the atom

c)

The "Plum Pudding Model" of the atom

d)

The "Quantum Mechanical Modell" of the atom

e)

The "Golf ball Model" of the atom

6.

John Dalton was the first person recorded as thinking that matter was ultimately composed of atoms.

a)

True

b)

False

7.

You can continually divide matter into smaller and smaller pieces without ever coming to an end.

a)

True

b)

False

8.

In all atoms, the number of protons is the same as the:

a)

mass number

b)

atomic number

c)

number of neutrons

9.

Any two atoms that have the same number of protons:

a)

have the same overall charge

b)

belong to the same element

c)

belong to the same isotope

d)

have the same mass number

10.

How many electrons does an Iodine atom have?

a)

53

b)

126

c)

73

d)

179

11.
The mass number of an element that has 18 protons, 18 electrons, and 19 neutrons is _____.
a)
12.5
b)
13
c)
25
d)
37
12.
What element has 42 protons?
a)
Ca
b)
Mo
c)
Zr
d)
Po
13.
If an atom of nickel has a charge of +3, how many electrons does the atom have?
a)
28
b)
25
c)
26
d)
31
14.
What quantities vary between isotopes of an element?
a)
protons, electrons, and atomic mass
b)
protons, electrons, and atomic number
c)
neutrons and electrons
d)
neutrons and atomic mass
15.
24.1% of all the isotopes of a an element have a mass of 75.23 amu, 48.7% have a mass of 74.61 amu, and 27.2% have a mass of 75.20 amu.
What is the average mass of this element?
a)
74.92 amu
b)
24.97 amu
c)
75.01 amu
d)
74.51 amu
16.

An element has three isotopes. Given the abundances and relative masses, calculate the average atomic mass and determine (from the periodic table) which element it is.


Abundances | Relative masses

0.005% | 234.04 amu

0.720% | 235.04 amu

99.275% | 238.05 amu

a)

Uranium (#92, Atomic Mass: 238.03 amu)

b)

Fluorine (#9, Atomic Mass: 19.00 amu)

c)

Mercury (#89, Atomic Mass: 200.59 amu)

d)

Polonium (#84 209 amu)

17.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
18.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
19.
What atom matches this electron configuration?
[Xe] 6s25d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
20.

This orbital diagram represents

a)

Sodium

b)

Magnesium

c)

Aluminum

d)

Iron

21.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
22.

Elements in group 1 of the periodic table are commonly referred to as what?

a)

Halogens

b)

Noble Gases

c)

Alkali Metals

d)

Alkaline Earth Metals.

23.

Elements in group 2 of the periodic table are commonly referred to as what?

a)

Halogens

b)

Noble Gases

c)

Alkali Metals

d)

Alkaline Earth Metals.

24.

Elements in group 17 of the periodic table are commonly referred to as what?

a)

Halogens

b)

Noble Gases

c)

Alkali Metals

d)

Alkaline Earth Metals.

25.

Elements in this group classification tend to be poor electrical and thermal conductors.

a)

Metalloids

b)

Transition metals

c)

Nonmetals

d)

Rare earth metals

26.

Elements in this group classification tend to have properties that are partially like metals and partially like non-metals such as the quality of semi-conductivity.

a)

Metalloids

b)

Transition metals

c)

Nonmetals

d)

Rare earth metals

27.

Which of the following is not a property of metals?

a)

brittle (can break apart easily)

b)

malleable (can bend, be formed into shapes)

c)

lustrous (shiny!)

d)

conduct heat and electricity

28.

Which two elements have the most similar chemical properties?

a)

K and Na

b)

K and Ca

c)

K and Cl

d)

K and S

29.

The elements that display the greatest nonmetallic character are located toward which corner of the periodic table?

a)

Dead center

b)

Lower left

c)

Lower right

d)

Upper left

e)

Upper right

30.

The elements K, Ca, Se+, Kr, and Ga− all appear in Period 4 of the Periodic Table.  Which arrangement, from left to right, orders them with respect to their atomic size, from largest to smallest?

a)

K; Ca; Se+; Kr; Ga

b)

Ca; Ga; K, Kr; Se

c)

K; Kr; Se; Ca; Ga

d)

K; Ca; Ga; Se; Kr

31.

Which list arranges the elements Na, Li, K, Rb, and Cs in order of increasing ionization energy (from left to right)?

a)

Cs; Rb; K; Na; Li

b)

Cs; Li; Na; K; Rb

c)

Na; Li; K; Rb; Cs

d)

Li; Na; K; Rb; Cs

32.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
33.

Which element in period 4 has the highest electronegativity?

a)

potassium

b)

calcium

c)

copper

d)

bromine

34.
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
35.

Which of the following halogens has the greatest electronegativity?

a)

Chlorine (Cl)

b)

Bromine (Br)

c)

Iodine (I)

d)

Astatine (At)

36.

Definition of ionization energy is

a)

The energy required to remove an electron

b)

The energy required to add an electron

c)

The ability to attract an electron

d)

The distance from the nucleus to the outermost electron

37.

Consider the group 1A element sodium (atomic number 11), the group 3A element aluminum (atomic number 13), and the group 7A element chlorine (atomic number 17). These elements are in period 3. How are the first ionization energies of these elements related? (least to greatest)

a)

sodium > aluminum > chlorine

b)

sodium < aluminum < chlorine

c)

sodium < chlorine < aluminum

d)

sodium > chlorine > aluminum

38.

What is the chemical formula for a compound formed between Sodium and Fluorine?

a)

NaF2

b)

Na2F2

c)

NaF

d)

Na2F

39.

What is the name for AlN?

a)

Aluminum Nitride

b)

Aluminum Nitrate

c)

Aluminum Nitrite

d)

Aluminum Oxide

40.

What is the charge on iron in FeO?

a)

+2

b)

+3

c)

+4

d)

+1

41.

What type of elements form anions?

a)

Metals

b)

Nonmetals

c)

Transition Elements

d)

Isotopes

42.

What is the chemical formula for a compound that forms between magnesium and sulfur?

a)

MgS

b)

Mg2S2

c)

Mg2S

d)

MgS2

43.

What is the chemical formula for barium iodide?

a)

Ba2I

b)

BaI

c)

BaI2

d)

BI

44.

if METALS are more likely to LOSE electrons, they will form ...

a)

anions

b)

neutral atoms

c)

cations

45.

Ionic compounds conduct electricity when dissolved in water. Which statement below best explains the property?

a)

Ions are free to move.

b)

Electrons are free to move.

c)

Bonds are strong.

d)

There are weak intermolecular forces of attraction.

46.
Which of the following is a property of an ionic compound?
a)
high melting point
b)
soft
c)
malleable
d)
liquid at room temperature
47.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

48.

S2O4S_2O_4  

a)

sulfur oxide

b)

disulfur pentaoxide

c)

disulfur tetraoxide

d)

disulfide tetraoxide

49.

nitrogen tribromide

a)

NBrNBr  

b)

N3BrN_3Br  

c)

NBr3NBr_3  

d)

N3BrN3Br  

50.

Each contains polar bonds but only one is a polar molecule

a)

CO2

b)

NH3

c)

CCl4

d)

CH4

51.

The shape of a molecule with 4 pairs of bonding electrons

a)

linear

b)

tetrahedral

c)

trigonal planar

d)

trigonal pyramidal

52.

Which molecule has only single bonds?

a)

CO2

b)

Cl2

c)

CO

d)

N2

53.

A bond formed between two bromine atoms is likely to be

a)

Ionic

b)

Coordinate covalent

c)

Polar

d)

Nonpolar

54.

Which of the following is a property of covalent compounds?

a)

Composed of a metal and nonmetal

b)

Low melting points

c)

Can conduct electricity when dissolved in water

d)

Typically solid at room temperature

55.

What is happening with the electrons in a nonpolar covalent bond?

a)

Electrons are being transferred from one atom to another

b)

Electrons are being shared unequally

c)

Electrons are being shared equally

d)

Nothing is happening to the electrons

56.

Which image could be a representation of NH3?

a)

A

b)

B

c)

C

57.

3. Which is a correct Lewis structure for hydrogen cyanide, HCN?

a)
b)
c)
d)
58.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

59.

What is the name of the ion with the formula C2H3O2-?

a)

Bromide

b)

Acetate

c)

Carbonate

d)

Cyanide

60.

Which ion has the formula H2PO4-?

a)

Phosphate

b)

Dihydrogen phosphate

c)

Oxalate

d)

Permanganate

61.
What is the MOLECULAR geometry of the central oxygen?
a)
Linear
b)
Trigonal Planar
c)
Bent
d)
Tetrahedral
62.
What is the best explanation of VSEPR theory?
a)
It explains the shapes that electrons make around atoms when they repel
b)
It explains how many electrons fit into an element's valent shell
c)
It explains why electrons pair up
d)
It explains why electrons repel each other
63.
Which molecule would have this molecular geometry?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
64.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
65.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
66.

Which one of the following is the correct bond angle between atoms adopting a trigonal planar geometry?

a)

180°

b)

109.5°

c)

90°

d)

120°

67.

Ammonia, NH3, adopts a tetrahedral geometry. However, the non-bonding pair on the central nitrogen atom distorts the bond angle away from the expected 109.5°. Which of the following statements correctly describes how the bond angle is distorted?

a)

The actual bond angle is reduced: it is less than 109.5°

b)

The actual bond angle is increased: it is more than 109.5°

68.

What shape is shown here?

a)

Octahedral

b)

Tetrahedral

c)

Trigonal bipyramidal

d)

Seesaw

69.
What molecule could this be? 
a)
H2O
b)
CCl4
c)
PCl5
d)
NaCl
70.

water H2O would have what kind of electron geometry

a)

linear

b)

trigonal planar

c)

tetrahedral

d)

bent

71.
What is the correct formula for Sodium Oxide?
a)
NaO
b)
NaO2
c)
Na2O
d)
Na2O2
72.
What kind of bond forms between a cation and an anion?
a)
Chemical bond
b)
Ionic bond
c)
Covalent bond
d)
Electron bond
73.
Which is the correct formula for aluminum oxide?
a)
AlO
b)
AlO2
c)
Al2O3
d)
Al3O2
74.
Name the following ionic compound: LiNO3
a)
lithium nitrate
b)
lithium III nitrate
c)
lithium nitride
d)
lithium oxide
75.
Name the following ionic compound: MgSO4
a)
magnesium sulfoxide
b)
magnesium sulfide
c)
magnesium sulfate
d)
magnesium oxide
76.
What is the charge on the hydroxide ion?
a)
0
b)
-1
c)
-2
d)
-3
77.
What is the correct formula for Sodium Oxide?
a)
NaO
b)
NaO2
c)
Na2O
d)
Na2O2
78.
What is the charge on the calcium ion?
a)
1+
b)
2+
c)
2-
d)
1-
79.
The correct chemical formula for magnesium phosphide is
a)
MgP
b)
Mg₂P₃
c)
Mg₃P₂
d)
Mg₃(PO₄)₂
80.

The key step in the formation of ionic compounds is ...

a)

electron transfer from nonmetal to metal atoms to form oppositely charged ions which are attracted to each other

b)

electron transfer from metal to nonmetal atoms to form oppositely charged ions which repel each other

c)

electron transfer from nonmetal to metal atoms to form oppositely charged ions which repel each other

d)

electron transfer from metal to nonmetal atoms to form oppositely charged ions which attract each other

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