Exam 3-5
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184 Terms
The smallest particle of an element that retains the characteristics of the element is a(n)
atom.
electron.
neutron.
nucleus.
proton.
atom
The primary substances of which all other things are composed are
compounds.
protons.
molecules.
electrons.
elements.
elements
What elements are in hydroxyapatite, Ca5(PO4)3OH , a major compound in human bones and teeth?
carbon, phosphorus, oxygen, helium
carbon, potassium, oxygen, helium
carbon, potassium, oxygen, hydrogen
calcium, phosphorus, oxygen, helium
calcium, phosphorus, oxygen, hydrogen
calcium, phosphorus, oxygen, hydrogen
sodium
No
Sm
So
Na
Au
Na
iron
Ir
FE
In
Fs
Fe
Fe
aluminum
Sn
Ag
Au
Am
Al
Al
silver
AG
Si
Au
S
Ag
Ag
potassium
Ko
P
K
Pt
Po
K
Au is the symbol for
gold.
aluminum.
silver.
argon.
sodium.
Gold
Which of the following is a characteristic of the modern periodic table?
The A groups contain the transition elements.
A group is a horizontal row on the periodic table.
The elements in each group have similar chemical properties.
The B groups contain the representative elements.
A period is a column on the periodic table.
The elements in each group have similar chemical properties.
What is the symbol of the element in Group 4A(14) and Period 2?
Ca
Mg
C
Si
Be
C
Identify the metalloid in the following list.
fluorine
copper
germanium
silver
sulfur
Germanium
The elements sodium, magnesium, and silicon
are in the same group.
are in the same period of elements.
have the same mass number.
have the same number of neutrons.
are isotopes of each other.
are in the same period of elements
What is the symbol of the element in Period 4 and Group 2?
C
Mg
Ca
Be
Si
Ca
Which of the following properties is NOT a characteristic of the Group 1A(1) elements (alkali metals)?
They are good conductors of heat.
They react vigorously with water.
Most of them are liquids at room temperature.
They are good conductors of electricity.
They are shiny.
Most of them are liquids at room temperature
Identify the noble gas in the following list.
oxygen
gold
nitrogen
chlorine
helium
helium
The elements lithium, sodium, and potassium
are isotopes of each other.
are in the same period of elements.
are in the same group.
have the same number of neutrons.
have the same mass number.
are in the same group
Which of the following is a characteristic of nonmetals?
good conductors of electricity
malleable
good conductors of heat
shiny
low melting points
low melting points
Which of the following elements is a noble gas?
argon
bromine
oxygen
chlorine
nitrogen
argon
Which element would have physical and chemical properties similar to chlorine?
O
Ar
P
S
Br
Br
Which of the following elements is a nonmetal?
nitrogen
iron
sodium
calcium
silver
nitrogen
The Group 8A(18) elements
melt at high temperatures.
are good conductors of electricity.
react vigorously with water.
are liquids at room temperature.
are unreactive and are rarely found in combination with other elements.
are unreactive and are rarely found in combination with other elements.
Which of the following elements is a metal?
strontium
phosphorus
argon
fluorine
nitrogen
strontium
The element in this list with chemical properties similar to magnesium is
boron.
chlorine.
carbon.
strontium.
sodium.
strontium
Semiconductors are located in the periodic table on (or in) the
line dividing metals from nonmetals in the table.
right side of the table.
last period of the table.
left side of the table.
first period of the table.
line dividing metals from nonmetals in the table.
According to Dalton’s Atomic Theory,
all atoms are different.
all matter is made up of tiny particles called electrons.
a compound can contain different numbers of atoms as long as it has the same kinds of atoms.
atoms are neither created nor destroyed during a chemical reaction.
atoms of the same element combine to form compounds.
atoms are neither created nor destroyed during a chemical reaction.
Which of the following descriptions of a subatomic particle is correct?
A neutron has a positive charge and a mass of approximately 1 amu.
An electron has a negative charge and a mass of approximately 1 amu.
A proton has a positive charge and a mass of approximately 1 amu.
A neutron has no charge and its mass is negligible.
A proton has a positive charge and a negligible mass.
A proton has a positive charge and a mass of approximately 1 amu.
In an atom, the nucleus contains
only neutrons.
an equal number of protons and electrons.
only protons.
all the protons and electrons.
all the protons and neutrons
all the protons and neutrons
Which of the following gives the correct numbers of protons, neutrons, and electrons in a neutral atom of Sn?
68 protons, 68 neutrons, 50 electrons
118 protons, 50 neutrons, 118 electrons
50 protons, 68 neutrons, 50 electrons
118 protons, 118 neutrons, 50 electrons
50 protons, 50 neutrons, 50 electrons
50 protons, 68 neutrons, 50 electrons
The mass number of an atom can be calculated from
the number of protons.
the number of protons plus neutrons.
the number of electrons.
the number of neutrons.
the number of electrons plus protons.
the number of protons plus neutrons.
The atomic number of an atom is equal to the number of
electrons plus protons.
neutrons.
nuclei.
neutrons plus protons.
protons.
protons
The number of neutrons in an atom is equal to
the atomic number.
the mass number.
the mass number - the atomic number.
the mass number + the atomic number.
the number of protons.
the mass number - the atomic number
Consider a neutral atom with 41 protons and 49 neutrons. The atomic number of the element is
41
Consider a neutral atom with 2 protons and 35 neutrons. The mass number for this atom is
37
What is the mass number of an atom of potassium that has 20 neutrons?
15
59
39
35
19
39
Consider a neutral atom with 51 protons and 61 neutrons. The number of electrons in this atom is
51
Isotopes are atoms of the same element that have
the same atomic mass but different numbers of protons.
the same atomic numbers but different numbers of electrons.
the same atomic numbers but different numbers of protons.
different atomic numbers.
the same atomic number but different numbers of neutrons.
the same atomic number but different numbers of neutrons.
The atomic mass of an element is equal to
one-twelfth of the mass of a carbon-12 atom.
a weighted average mass of all of the naturally occurring isotopes of the element.
the average mass of all of the naturally occurring isotopes of the element.
its mass number.
its atomic number.
a weighted average mass of all of the naturally occurring isotopes of the element.
How many protons are in an isotope of sodium with a mass number of 25?
14
15
11
32
25
11
Which of the following is NOT true for the atoms 13N, 14N, and 15N?
They all have the same mass number.
They are isotopes.
They all have 7 protons.
They all have 7 electrons.
They all have the same atomic number.
They all have the same mass number.
The correct symbol for the isotope of potassium with 22 neutrons is
40/19 K
none of the answers are correct.
41/ 19 K
39/19 K
22/19 K
41/19 k
Consider an isotope of sodium with a mass number of 25. The number of neutrons in this isotope of sodium is
32.
16.
14.
25.
11.
14
A sample of silicon has three naturally occurring isotopes: Si-28 (mass 28.0 amu); Si-29 (mass 29.0 amu) and Si-30 (mass = 30.0 amu). If the average atomic mass of silicon is 28.1 amu, which isotope is the most abundant?
Si-28
Si-29
All isotopes have the same natural abundance.
Si-30
Si-28
The electron arrangement of any particular atom shows
a diagram of an atomic nucleus.
a description of the shape of each energy level.
the maximum number of electrons each energy level can hold.
the number of isotopes possible.
the number of electrons in each energy level.
the number of electrons in each energy level.
What is the abbreviated electron configuration for nickel (atomic number 28)?
[Ar]4s24p4
[Ar]4s23d8
[Kr]4s23d8
[Ar]3d8
[He]2s22p3
[Ar]4s23d8
What is the electron configuration for aluminum?
1 s22s22p63s23p6
1 s22 s22p63s23p8
1 s22s22 p63s23p1
1 s22s22p63s23p5
1 s22s22p63s23p3
1 s22s22 p63s23p1
What is the electron configuration for potassium (atomic number 19)?
1s22s22p63s23p54s1
1s22s22p63s23p64s1
1s22s22p83s23p5
1s22s22p63s23p7
1s22s22p63s23p53d2
1s22s22p63s23p64s1
What is the element with the abbreviated electron configuration [Kr]5s24d8?
Kr
Pt
Pd
Ni
Xe
Pd
What is the element with the electron configuration 1s22s22p63s23p5?
S
Be
F
Ar
Cl
Cl
Which of the following electron configurations is impossible?
1s22s22p63s23p6
1s22s22p63s23p1
1s22s22p63s23 p5
1s22s22p63s23p3
1s22 s42p63s23p3
1s22 s42p63s23p3
What element has the electron configuration 1s22s22p63s23p2?
iron
oxygen
silicon
carbon
sulfur
silicon
What is the correct electron configuration for the lithium atom?
2s1
1s3
1s22s5
1s12s2
1s22s1
1s22s1
The maximum number of electrons that may occupy energy level n= 2 is?
8
8
In an electron-dot structure of an element, the dots are used to represent
only the electrons that will participate in bond formation.
all of the electrons in the atom.
the electrons that the element will gain when it forms a compound.
the electron arrangement.
the valence electrons.
the valence electrons
The number of electron levels in a magnesium atom is
1.
5.
2.
4.
3.
3
Valence electrons are electrons located
in the innermost energy level of an atom.
in the outermost energy level of an atom.
throughout the atom.
in the first three shells of an atom.
in the nucleus of an atom.
in the outermost energy level of an atom.
The number of dots in the electron dot structure of nitrogen is
one.
three.
five.
two.
four.
five
The number of valence electrons found in an atom of a Group A element is equal to
its mass number.
its atomic number.
eight minus the group number.
eight.
its group number
its group number
How many valence electrons are in the electron-dot structures for the elements in group 2A?
2
The number of electrons in the outer energy level of a neutral atom of boron (atomic number 5) is
5.
8.
10.
3.
2.
3
The atomic size of atoms
decreases going across a period.
increases going across a period.
decreases going down within a group.
does not change going across a period.
None of the above.
decreases going across a period.
Of the elements: B, C, F, Li, and Na., the element with the largest atomic radius is
Li.
B.
F.
C.
Na.
Na
Of the elements: B, C, F, Li, and Na, the element with the smallest atomic radius is
C.
F.
Na.
Li.
B.
F
The ionization energy of atoms
None of the above.
decreases going across a period.
increases going down within a group.
decreases going down within a group.
does not change going down within a group.
decreases going down within a group
Ionization energy is
None of the above.
the energy needed to remove the least tightly bound electron.
higher for potassium than for lithium.
highest for metals in Group 1A (1).
the energy an ion acquires from an electron.
the energy needed to remove the least tightly bound electron
Of the elements: B, C, F, Li, and Na. The element with the highest ionization energy is
C.
Na.
B.
F.
Li.
F
Of the elements: B, C, F, Li, and Na. The element with the smallest ionization energy is
F.
Li.
B.
C.
Na.
Na
Of the elements: B, C, F, Li, and Na. The element with the least metallic character is
B.
Li.
Na.
F.
C.
F
Of the elements: B, C, F, Li, and Na. The element with the most metallic character is
F.
Li.
C.
B.
Na.
Na
A(n) __________ is the smallest neutral unit of two or more atoms held together by a covalent bond.
molecule
Valence electrons are electrons located
throughout the atom.
in the outermost energy level of an atom.
in the nucleus of an atom.
in the innermost energy level of an atom.
in the first three shells of an atom.
in the outermost energy level of an atom.
What it the main difference between an ionic and a covalent bond?
Both bonds are the same, but named different to describe different atoms involved.
One is the sharing of a pair of electrons, the other is the transfer of at least one electron.
One involves electrons, the other does not involve any electrons.
The electrons are traded between the two atoms and this keeps the atoms close.
The electrons in both types of bonding undergo an exchange.
One is the sharing of a pair of electrons, the other is the transfer of at least one electron.
An anion always
has a negative charge.
contains a group of two or more atoms with a positive charge.
contains a metal and a nonmetal.
forms covalent bonds.
has a positive charge.
has a negative charge
Which of the following does not describe ionic compounds?
They are usually very ordered.
They are held together by electrostatic attraction.
They have a tendency to melt easily.
They consist of positive and negative ions.
none of the above
They have a tendency to melt easily.
Which of the following compounds contains an ionic bond?
CH 4
H 2O
CaO
H 2
NH 3
CaO
In ionic compounds, __________ lose their valence electrons to form positively charged __________. (5,2)
nonmetals; anions
metals; anions
metals; cations
nonmetals; cations
metals; polyatomic ions
metals; cations
Which of the following molecules contains an ionic bond?
Cl 2
MgCl 2
Cl 2O 7
SF 3
none of the above
MgCl2
Which of the following compounds would be ionic?
CS2
CaCl2
CF4
SF5
SO2
CaCl2
Which of the following compounds contains ionic bonds?
Cl2
K2O
CH4
OF2
none of the above
K2O
In a molecule with covalent bonding,
atoms of metals form bonds to atoms of nonmetals.
atoms of different metals form bonds.
atoms are held together by sharing electrons.
atoms of noble gases are held together by attractions between oppositely charged ions.
oppositely charged ions are held together by strong electrical attractions.
atoms are held together by sharing electrons.
Ionic bonding is expected in which of these compounds?
OF2
KF
Cl2
H2
HF
KF
Which of the following would be a negative ion with a single charge?
an atom with 11 protons and 12 electrons
an atom with 10 protons and 12 electrons
an atom with 12 protons and 11 electrons
an atom with 11 protons and 11 electrons
none of the above
an atom with 11 protons and 12 electrons
Elements in group 2A(2) of the periodic table form ions with a charge of
3+.
0.
1+ .
1- .
2+ .
2+
The number of electrons in the highest energy level of nitrogen is
one.
two.
three.
four.
five.
five
The number of electrons in an ion with 20 protons and an ionic charge of 2+ is
20.
16.
22.
24.
18.
18
What is the symbol for the ion with 19 protons and 18 electrons?
F-
Ar+
F+
K-
K+
K+
What is the ionic charge of an ion with 13 protons and 10 electrons?
3-
3+
2-
2+
1+
3+
Which of the following elements has six valence electrons?
N
B
C
Be
O
O
The octet rule indicates that
all of the Group A elements have 8 valence electrons.
atoms lose, gain, or share valence electrons to have 8 valence electrons.
all of the shells in an atom hold a maximum of 8 electrons.
all of the noble gases have eight total electrons.
the noble gases react with other compounds to get 8 valence electrons.
atoms lose, gain, or share valence electrons to have 8 valence electrons.
The number of valence electrons found in an atom of a Group A element is equal to
its group number.
eight.
its mass number.
its atomic number.
eight minus the group number.
its group number
If a neutral atom gains two electrons, what is the electrical charge of the atom?
+2
neutral
-1
-2
+1
-2
How many valence electrons are in the electron-dot structures for the elements in group 3A(13)?
1
2
3
4
6
3
How many valence electrons does bromine (Br, atomic no. = 35) have?
21
28
35
1
7
7
How many valence electrons does gallium (Ga, atomic no. = 31) have?
1
31
6
70
3
3
How many valence electrons does boron (B, atomic no. = 5) have?
1
2
3
4
5
3
How many electrons will aluminum gain or lose when it forms an ion?
gain 5
gain 1
lose 3
lose 2
lose 1
lose 3
Which of the following elements has two valence electrons?
Mg
Li
Ne
Na
H
Mg
What needs to be done to convert a neutral nitrogen atom into an N3- species?
add three protons
add three nitrogens
add three electrons
remove three electrons
remove three protons
add three electrons
The number of electrons in the highest energy level of carbon is
one.
two.
three.
four.
five.
four
An ionic compound
has a net negative charge.
contains only cations.
has a net charge of zero.
contains only anions.
has a net positive charge.
has a net charge of zero
Note 
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