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Unit 1_Honors Chemistry I

Total questions: 80

Worksheet time: 48mins

Name
Class
Date
1.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

2.

Subatomic particles found on the outermost shell & responsible for the atom's reactivity

a)

neutrons

b)

valence electrons

c)

isotopes

d)

ions

3.
Value representing the number of protons in an element
a)
Atomic Mass
b)
Mass Number
c)
Valence Electrons
d)
Atomic Number
4.
A tiny but very dense, positively charged portion of the atom that holds most of the atomic mass
a)
Electron Shells
b)
Orbitals
c)
Electron Cloud
d)
Nucleus
5.
Calculation used to find the number of neutrons in an atom
a)
Atomic Mass - Atomic Number
b)
Atomic Number - Atomic Mass
c)
Atomic Mass - Electrons
d)
none of these
6.

The only element with typically has no neutrons in its nucleus.

a)

Oxygen

b)

Helium

c)

Hydrogen

d)

Lithium

7.
The nucleus of an atom is made of
a)
electrons and protons
b)
electrons and neutrons
c)
protons and neutrons
d)
empty space
8.
Most of the volume an atom is made of this
a)
the nucleus
b)
the protons
c)
the neutrons
d)
empty space
9.

What is the number of protons that the element in this image contains?

a)

14

b)

7

c)

15

d)

18

10.

What is the atomic number of this atom?

a)

1

b)

3

c)

4

d)

7

11.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

12.
In order for an atom to be neutral what has to be true?
a)
The atom has more protons than neutrons
b)
The atom has more neutrons than protons
c)
The atom has the same number of protons and neutrons
d)
The atom has the same number of protons and electrons
13.

An atom has 10 protons, 15 neutrons and 10 electrons what is its mass number.

a)

20

b)

10

c)

35

d)

25

14.

Which element is represented by the image?

a)

Boron

b)

Carbon

c)

Nitrogen

d)

Oxygen

15.

An element with an atomic number of 5 and a mass number of 11 has many neutrons?

a)

11

b)

5

c)

6

d)

16

16.

Of the following sublevels, which is the highest in energy?

a)

4s

b)

3d

c)

4d

d)

5s

17.

Which electron transition releases a photon with the greatest energy?

a)

orbital 6 to orbital 3

b)

orbital 5 to orbital 3

c)

orbital 4 to orbital 3

d)

orbital 7 to orbital 3

18.

Which of these has the shortest wavelength?

a)

infrared

b)

yellow light

c)

microwaves

d)

blue light

19.

Emission spectra (bright line spectra) are created when electrons move from ___.

a)

higher to lower energy levels.

b)

lower to higher energy levels.

c)

s orbitals to p orbitals.

d)

one atom to a different atom.

20.

All forms of EM radiation travel at the same speed and have the same energy.

a)

False, they travel at the same speed but have different energies

b)

True

c)

False, they travel at different speeds but have the same energy

21.

The analysis of the way matter emits and absorbs radiation is called ___.

a)

astronomy

b)

chemistry

c)

spectroscopy

d)

atomic theory

22.

Each element on the periodic table can be identified by its

a)

classification as a solid, liquid or gas.

b)

metallic properties.

c)

ability to react to form compounds.

d)

unique spectral "fingerprint."

23.
Light is emitted when electrons ...
a)
jump from high to low 
b)
jump from low to high 
c)
either of these
d)
none of these
24.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Helium

25.

Of the following orbitals, which has the lowest energy and would therefore fill first?

a)

4s

b)

3d

c)

4p

d)

48

26.

What charge does an ion have when it GAINS electrons?

a)

Positive

b)

Negative

c)

Neutral

27.

How many neutrons does this bromine atom have?

a)

35

b)

45

c)

80

d)

115

28.

What two particles determine the mass number?

a)

Protons and electrons

b)

Electrons and neutrons

c)

Protons and neutrons

29.

What differs between an atom and an ion of the same element?

a)

The number of electrons

b)

The number of protons

c)

The number of neutrons

30.

What is the representation of an isotope?

a)

N3-

b)

Al3+

c)

Si

d)

P-33

31.

How many neutrons does this Neon atom have?

a)

21

b)

11

c)

10

d)

12

32.

What is the mass number of this element?

a)

12

b)

24

c)

23

d)

11

33.

What is the charge on a lithium atom that loses 1 electron?

a)

+1

b)

0

c)

-1

d)

-2

34.
When an atom loses a valence electron, it becomes a(n) _____________ ion.
a)
positive
b)
negative
c)
neutral
d)
polyatomic
35.

What is the number of protons, neutrons, and electrons?

a)

16,34,16

b)

16,18,16

c)

16,16,18

d)

16.18.18

36.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
37.

What charge would an ion of calcium have?

a)

+1

b)

+2

c)

-1

d)

-2

38.
If an element has 3 valence electrons, what charge will likely form on its ion ?
a)
+3
b)
+5
c)
-3
d)
-5
39.

Which of the following has an ion with a -3 charge?

a)

Boron

b)

Fluorine

c)

Nitrogen

d)

Neon

40.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
41.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
42.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
43.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
44.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
45.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
46.

The 4 orbitals are

a)

s, p, d, f

b)

a, b, c, d

c)

2, 4, 6, 8

47.

How many p orbitals are there in the 2nd energy level? (Remember that each orbital holds 2 electrons.)

a)

2

b)

1

c)

4

d)

3

48.

What is the shorthand electron configuration for Sulfur atom?

a)

[Ar] 3p4

b)

[He] 3s23p4

c)

[Ne] 3s23p4

d)

[Na] 3s23p3

49.
What noble gas should be used to write the shorthand configuration for Te?
a)
Ar
b)
Kr
c)
Xe
d)
Sb
50.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
51.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
52.
Which orbital has the least amount of energy? 
a)
p orbital
b)
d orbital
c)
s orbital 
d)
What is an orbital?
53.

Electrons fill energy levels and sublevels _____ in energy first.

a)

lower

b)

higher

54.

Of the following sublevels, which is the highest in energy?

a)

4s

b)

3d

c)

4p

d)

5s

55.

Name the element- 1s2 2s2 2p6 3s2 3p6 4s2 3d5

a)

Manganese

b)

Magnesium

c)

Aluminum

d)

Boron

56.
Most of the nonmetals on the periodic table are located...
a)
on the left side
b)
at the bottom
c)
on the right side
d)
in the middle
57.
In the modern periodic table, elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
58.
_______ are the ROWS on the periodic table.
a)
Families
b)
Groups
c)
Periods
d)
Elements
59.
________ are the COLUMNS on the periodic table and are organized by similar properties.
a)
Classifications
b)
Groups
c)
Periods
d)
Elements
60.
Atoms with similar properties are most likely located...
a)
in the same period.
b)
in the same group.
c)
in different periods.
d)
to the right and left of each other.
61.
The yellow atoms are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
62.
Which elements have the most similar chemical properties?
a)
K and Na
b)
K and Ca
c)
K and Cl
d)
K and S
63.
Rows on the period table are called _____ while columns are called _____.
a)
groups, families
b)
groups, periods
c)
periods, groups
d)
families, groups
64.
The periodic table has __ groups.
a)
8
b)
7
c)
18
d)
2
65.

Based on its position on the periodic table, Carbon has __ orbitals and __ valence electrons.

a)

4,2

b)

2.4

c)

2,6

d)

6,2

66.

what is the name of group number 1

a)

halogens

b)

noble gases

c)

alkali metals

d)

alkaline earth metals

67.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
68.

Which element is not a metal?

a)

Na

b)

K

c)

Al

d)

Si

69.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
70.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
71.

What causes an element to have higher electronegativity ?

a)

more orbitals with more protons

b)

more orbitals with fewer protons

c)

fewer orbitals with more protons

d)

fewer orbitals with fewer protons

72.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
73.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
74.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more neutrons
75.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
76.
Electronegativity is...
a)
the ability of an atom to attract/ accept electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
77.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
78.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
79.
Metals have the largest - 
a)
atomic radius and electronegativity
b)
electronegativity and ionization energy
c)
atomic radius only
d)
ionization energy and atomic radius
80.

Which statement correctly and completely identifies a trend?

a)

Atomic radius decreases across a period and increases down a group.

b)

Electronegativity decreases across a period and decreases down a group.

c)

Ionization energy increases across a period and increases down a group.

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