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10th Grade Mid-term Fall2024

Total questions: 85

Worksheet time: 3hrs 49mins

Name
Class
Date
1.
How many PERIODS does the Periodic Table have?
a)
1
b)
7
c)
8
d)
18
2.
Which PERIOD does Radon belong to? 
a)
18
b)
8
c)
6
d)
1
3.
Element from Period #2, Group #1?
a)
Lithium
b)
Beryllium 
c)
Helium 
d)
Lead
4.
Who has ATOMIC NUMBER 20?
a)
Calcium
b)
Neon 
c)
Carbon 
d)
Krypton
5.

The _________________ are a small group of elements that have both metallic and nonmetallic properties.

a)

Oxygen Group

b)

Nitrogen Group

c)

Metalloids

d)

Halogens

6.

The _______________electrons are the electrons on the outer most energy level of the atom.

a)

valence

b)

core

c)

excited

d)

ground state

7.

Group 18: Unreactive nonmetals. All are colorless, odorless gases at room temperature. These elements have a full outer energy level, usually 8 valence electrons, except for Helium which only has 2 valence electrons.

a)

Nitrogen Group

b)

Oxygen Group

c)

Noble Gases

d)

Halogens

8.

The ability of an atom to attract electrons is called __________.

a)

atomic radius

b)

ionization energy

c)

electronegativity

9.

Why does sulfur have a greater ionization energy than aluminum? (select all that apply)

a)

Sulfur has more electron shells

b)

Sulfur has more valence electrons

c)

Sulfur has a smaller atomic radius

d)

Sulfur has less protons

10.

Metals want to _____ electrons and are therefore left with a _______ charge.

a)

gain; positive

b)

gain; negative

c)

lose; positive

d)

lose; negative

11.

You have Mg, Ba, Be, and Ca. Which choice has the elements arranged from smallest to largest in atomic radius?

a)

Ba, Ca, Be, Mg

b)

Be, Ca, Ba, Mg

c)

Ca, Mg, Ba, Be

d)

Be, Mg, Ca, Ba

12.

You have the elements Ca, Ga, K and Br. Which element has the lowest electronegativity and why?

a)

K, furthest to the right on the PT

b)

Br, furthest to the right on the PT

c)

K, furthest to the left on the PT

d)

Br, furthest to the left on the PT

13.

You have the elements S, O, Te, Se. Which of these has the highest attraction of electrons of another element and why?

a)

O, furthest from Te, more rings means less attraction

b)

Se, closer to O, more rings means more attraction

c)

Te, furthest from O, more rings means more attraction

d)

O, furthest from Te, more rings means more attraction

14.
This model added on to previous models by showing electrons existed at certain "energy levels". However it does not accurately show what those levels look like.
a)
The "Bohr Model" of the atom
b)
The "Rutherford Model" of the atom
c)
The "Plumb Pudding Model" of the atom
d)
The "Quantum Mechanical Model" of the atom
15.
What does the nucleus of an atom contain?
a)
Electrons & Neutrons
b)
Protons & Neutrons
c)
Neutrinos & Positrons
16.
His atomic model included a dense positive core in an atom, surrounded by negatively charged particles
a)
Joseph Thomson
b)
Niels Bohr
c)
Ernest Rutherford
17.
A certain photon of light has a wavelength of 4.22x10-7nm. What is the frequency? (v=c/λ)
a)
7.11x1014 Hz
b)
7.11Hz
c)
1.41x10-15
d)
-1.41x1015
18.
Select the correct order of waves on the EMS 
a)
Radio, Micro, Infra, Visible, Ultra, X-ray, Gamma
b)
Gamma, X-ray, Ultra, Vis, Infra, Micro, Radio
c)
Vis, Micro, Infra, Ultra, X-ray, Gamma, Radio
d)
Micro, Radio, Vis, Infra, Ultra, X-ray, Gamma
19.
What is the energy of a quantum of light with a frequency of 7.39x1014Hz.(E=Hv)
a)
4.88x1019
b)
4.88x10-19
c)
2.22x1023
d)
2.22x10-23
20.
According to the Bohr Model, electrons are only found in specific orbits around the nucleus called __________________________
a)
Energy Levels
b)
Electron Lanes
c)
Electron Places
d)
Atomic Mass
21.

In which state does an electron have the least amount of energy?

a)

Excited state

b)

Ground state

c)

Orbital

d)

Bohr model

22.
The _______________ determines the color of visible light. 
a)
wavelength
b)
speed
c)
amplitude
d)
light
23.
When talking about energy levels in an atom, what is an "excited state"?
a)
The highest energy state of an atom.
b)
Any level higher than the ground state.
c)
The lowest energy state of an atom.
d)
When an atom loses an electron
24.

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

a)

3

b)

6

c)

8

d)

10

25.
What is the noble gas shorthand electron for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p4
26.

A packet of light is called

a)

An eon

b)

An electron

c)

A photon

d)

A quantum

27.

According to the graph above, which color of light has the shortest wavelength?

a)

Blue

b)

Green

c)

Purple

d)

Orange

28.

Which of the following BEST describes the purpose of electron configurations?

a)

To describe the location of electrons within the orbitals of an atom.

b)

To describe the location of protons within the orbitals of an atom.

c)

To show how many levels or "shells" an atom has.

d)

To calculate the total number of electrons in the atom.

29.

Which types of elements become cations?

a)

non-metals

b)

metals

c)

metalloids

30.
Nonmetals tend to 
a)
gain electrons
b)
lose electrons
31.

Which type of bond is formed from the sharing of electrons?

a)

ionic bond

b)

covalent bond

32.

Which set of elements is most likely to form an ionic compound?

a)

Na and O

b)

C and O

c)

Na and K

33.

Which of the following types of bonding results in materials which have the highest melting and boiling points?

a)

ionic bonding

b)

covalent bonding

34.

Sugar melts at a LOW temperature, it IS SOLUBLE in water, and WILL NOT conduct electricity.What type of bond does it have?

a)

Ionic Bond

b)

Polar Covalent Bond

c)

Nonpolar Covalent Bond

35.

Why are metals malleable? (They can bend without breaking.)

a)

Metals are very smooth.

b)

Metals have a sea of electrons.

c)

The sea of electrons form a strong metallic bond.

d)

Even though the metal ions repel each other, the electron sea holds all the atoms in place.

36.

The name of FeCl₂ is

a)

iron chloride

b)

iron(II) chloride

c)

iron(I) chloride

d)

iron dichloride

37.

Name the ionic compound SnSe2

a)

Tin diselenide

b)

Tin(IV) Selenide

c)

Tin selenide

d)

Tin(II) triselenide

38.

Name the following ionic compound: Cs2S

a)

cesium sulfide

b)

cesium sulfate

c)

cesium(II) sulfate

d)

cesium(II) sulfide

39.

When naming a compound, which of these is written first?

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

40.

What is the name of the following compound: CuBr2

a)

copper bromine

b)

copper bromide

c)

copper(I) bromide

d)

copper(II) bromide

41.

What is the what charge of lead in the compound: lead(IV) iodide

a)

+1

b)

+4

c)

+6

d)

-1

42.

Which is the correct formula for the compound: Calcium Oxide

a)

CaO

b)

CaO2

c)

Ca2O

43.
The chemical formula for an ionic compound of potassium and oxygen is
a)
KO.
b)
K2O.
c)
K2O2.
d)
KO2.
44.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

45.

When naming a compound, which of these is written first?

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

46.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
47.
What is the name of Br6F10 ?
a)
Bromium fluoride
b)
Hexabromine fluoride
c)
Bromium decafluoride
d)
none of the above
48.
What is the correct name for C4H6?
a)
Carbon Hexahydride
b)
Pentacarbon Pentahydride
c)
Hexacarbon Tetrahydride
d)
Tetracarbon Hexahydride
49.
What VSEPR shape is this
a)
Linear
b)
Line
c)
Tetrahedral
d)
Bent
50.
Why is H2O bent?
a)
left over electron pairs
b)
It has no carbon
c)
It is not bent, but linear
d)
Oxygen has 4 valence electrons
51.
What VSEPR structure would O2 form?
a)
Linear
b)
H-7
c)
Gas
d)
Bent
52.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
53.

Which of the following shapes can have unshared pairs of electrons on the central atom?

a)

trigonal pyramidal

b)

Bent

c)

Trigonal Planar

d)

Tetrahedral

e)

Linear

54.

Determine the molecular geometry of the given structure.

a)

Trigonal Pyramidal

b)

Bent

c)

Trigonal Planar

d)

Tetrahedral

55.

What intermolecular forces would exist between molecules of HF?

a)

London Dispersion Forces

b)

Dipole-Dipole Forces

c)

Hydrogen Bonding

d)

All of the above

56.

Which of the following would experience dipole-dipole forces of attraction between molecules?

a)
b)
c)
d)
57.

In a polar covalent bond, which atom will have a partial positive charge?

a)

The atom with the greater electronegitivity

b)

The atom that attracts more electrons

c)

The atom with the lower electronegativity

58.

What must the difference in electronegativity between two atoms be in order for the bond between them to be polar covalent?

a)

less than 0.4

b)

greater than 1.7

c)

between 0.4 and 1.7

d)

exactly 0

59.

Which describes this compound?

a)

Polar

b)

Non-polar

c)

Ionic

60.

The shape of BH3 molecule is trigonal planar but NH3 is trigonal pyramidal. Choose the best statement to describe the above observations

a)

Boron has larger atomic size than nitrogen

b)

Nitrogen has a lone pair whereas Boron does not

c)

Nitrogen is more electronegative than boron

d)

Boron is metalloid while nitrogen is non-metal

61.

In hydrogen chloride, the hydrogen atom is __________ charged whereas the chlorine atom is __________ charged.

a)

Partially positively; Partially negatively

b)

Partially negatively; Partially positively

62.

Describe the shape of the molecule.

a)

linear

b)

bent

c)

trigonal pyramidal

d)

tetrahedral

63.

What is Avogadro's number?

a)

6.02 x 1023

b)

1 mole

c)

600 million

d)

6.02

64.

How many moles are in 6.02 x 1023 molecules of H2O?

a)

1 mole

b)

2 moles

c)

6.02 moles

d)

602000000000000000000000 moles

65.

How many moles are in 8.30 X 1023 molecules of H2O?

a)

1.38 X 1023 moles H2O

b)

1.38 moles H2O

c)

2 moles H2O

d)

1 mole H2O

66.

What is the conversion factor that should be used to determine how many molecules are there in 4.00 moles of glucose, C6H12O6?

a)
b)
c)
d)
67.

What converting from moles to the number of particles, moles is multiplied by:

a)

an equivalent value

b)

a conversion factor

c)

the number of atoms in the formula

d)

the mass of the substance

68.

Why is the mole used in chemistry?

a)

The mass of atoms is in AMUs which is too hard to convert to grams.

b)

A dozen is not a scientific amount.

c)

Chemists needed to make chemistry easier to understand.

d)

It makes counting large numbers of small particles easier.

69.

How many moles are in 4.5 x 1024 atoms of lithium?

a)

2.71 x 1048 particles

b)

7.47 moles

c)

7.47 x 1024 atoms

d)

2.71 moles

70.

What are the units for Avogadro's number?

a)

meters

b)

particles

c)

grams

d)

liters

71.

How many grams is one mole of Sodium?

a)

32.07

b)

118.71

c)

150.36

d)

22.99

72.

How many moles are 156.00 grams of Chromium?

a)

4

b)

52

c)

3

d)

1

73.

What is the molar mass of (NH4)2CO3?

a)

144g

b)

138g

c)

96g

d)

78g

74.

What is the mass in grams of 5.90 mol C8H18?

a)

0.0512g

b)

19.4g

c)

389g

d)

673g

75.

You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.

a)

SO

b)

SO2

c)

SO3

d)

SO4

76.

What is the empirical formula for N2S3?

a)

NS

b)

N3S2

c)

N2S3

d)

N1S1.5

77.

Given the following: 42.07% Na, 18.89% P, and 39.04% O, determine the empirical formula.

a)

NaPO2

b)

Na2PO3

c)

Na3PO4

d)

NaPO4

78.
What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?
a)
C3H8
b)
CH4
c)
C2H2
d)
C4H10
79.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
80.
What is the percent composition by mass of oxygen in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
81.
Glycerol has a molar mass of 92.09g/mol. Its percent composition is: 39.12% C, 8.75% H, and 51.12% O. What is the molecular formula for glycerol?
a)
C2H3O2
b)
CH2O
c)
C2H4O2
d)
C3H8O3
82.

Determine the number of moles of Mg3P2 that are in 583 g of the compound.

a)

2.9 mol

b)

6.1 mol

c)

4.3 mol

d)

1.7 mol

83.
What is the mass of 0.75 moles of (NH4)3PO4?
a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g
84.

Carbon monoxide, a deadly gas, has a chemical formula of CO (one carbon atom with one oxygen atom). If you look at the total atomic mass of CO, does carbon or oxygen make up more of the mass?

a)

carbon

b)

oxygen

c)

they are exactly the same

d)

it is impossible to tell

85.

Lithium phosphide (three lithium atoms with one phosphorus atom) has a chemical formula of Li3P. If you look at the total atomic mass of Li3P, does lithium or phosphorus make up more of the mass?

a)

lithium

b)

phosphorus

c)

they are exactly the same

d)

it is impossible to tell

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