Semester 1 Review

The nucleus of most atoms is made up of:
1. protons and electrons
2. protons and neutrons
3. neutrons and electrons
4. electrons and protons
The charge and mass number of an electron are:
1. charge = +1, Mass number = 0
2. charge = -1, Mass number = 0
3. charge = 0, Mass number = 1
4. charge = +1, Mass number = 1
The mass number of an atom is determined by:
1. adding the protons and electrons
2. adding the neutrons and electrons
3. adding the neutrons and protons
4. the number of protons only
The _______________ constitute(s) most of the volume of an atom.
1. protons
2. neutrons
3. nucleus
4. electron cloud
How many electrons, neutrons and protons would be found in an atom of carbon-14 (atomic number 6)?
1. 6 electrons, 6 neutrons, 6 protons
2. 6 electrons, 6 neutrons, 8 protons
3. 8 electrons, 8 neutrons, 6 protons
4. 6 electrons, 8 neutrons, 6 protons
How many electrons would be found in an atom of oxygen (atomic number 8)?
1. 2
2. 4
3. 6
4. 8
The atomic number of an element is equal to:
1. the number of protons in the atom
2. the number of neutrons in the atom
3. the number of protons plus the number of neutrons
4. the number of protons plus the number of electrons
An element with nine protons in every atom must:
1. have nine neutrons as well
2. be fluorine
3. have a mass number of nine
4. be unstable
The laws of electrostatics consistently demonstrate that opposite charges:
1. destroy one another
2. attract
3. repel
Most of the mass of the atom can be found in the:
1. electron cloud
2. nucleus
3. electrons
4. charges
To four significant figures, the how many atoms are there in one mole of any element?
1. 2.06 x 10^-3
2. 6.02 x 10^-23
3. 6.022 x 10²³
4. 12.0
How many grams of naturally occurring phophorus must one have in order to have one mole of phosphorus?
1. 15 grams
2. 30.97 grams
3. 6.02 x 10²³ grams
4. 6.02 x 10^-23 grams
Which of the following descriptions does not apply to the nucleus?
1. Very dense
2. Mostly empty space
3. Positively charged
4. Very small
How many neutrons are there in an atom of hydrogen-3?
1. 0
2. 1
3. 2
4. 3
How many moles of magnesium are there in 48.62 grams of magnesium?
1. 0.5000 moles
2. 2.000 moles
3. 3.01 x 10²³ moles
4. 6.02 x 10²³ moles
What is the mass in grams of 3.50 moles of boron (at #5)?
1. 37.8 grams
2. 3.09 grams
3. 0.324 grams
4. 2.11 x 10²⁴ grams
The charge and mass number of a proton are:
1. charge = +1, Mass number = 0
2. charge = -1, Mass number = 0
3. charge = 0, Mass number = 1
4. charge = +1, Mass number = 1
The charge and mass number of a neutron are:
1. charge = +1, Mass number = 0
2. charge = -1, Mass number = 0
3. charge = 0, Mass number = 1
4. charge = +1, Mass number = 1
Of the basic atomic particles, the one that would be attracted to a negatively charged metallic plate is the:
1. proton
2. neutron
3. electron
Isotope Mass number Atomic number Protons Neutrons Electrons
Scandium-45
1. The blanks, respectively, would be filled: 21, 45, 21, 21, 24
2. The blanks, respectively, would be filled: 45, 21, 21, 24, 21
3. The blanks, respectively, would be filled: 21, 45, 24, 21, 21
4. The blanks, respectively, would be filled: 24, 21, 45, 21, 21
Isotope Mass number Atomic number Protons Neutrons Electrons
_______________-27 13
1. The blanks, respectively, would be filled: aluminum, 27, 13, 13, 14
2. The blanks, respectively, would be filled: cobalt, 40, 27, 13, 27
3. The blanks, respectively, would be filled: aluminum, 27, 13, 14, 13
4. The blanks, respectively, would be filled: silicon, 27, 14, 13, 13
An electron emitted from the nucleus during some kinds of radioactive decay is known as:
1. An alpha (a) particle
2. A beta (b) particle
3. A positron
4. A gamma ray
An alpha (a) particle is essentially a ____________________ nucleus.
1. hydrogen
2. uranium
3. carbon-12
4. helium
5. plutonium
Gamma (g) rays are:
1. are very high energy, very short wavelength electromagnetic radiation
2. are very high energy, very long wavelength electromagnetic radiation
3. are very low energy, very short wavelength electromagnetic radiation
4. are very low energy, very long wavelength electromagnetic radiation
Very large nucei tend to be unstable because of the:
1. repulsive forces between electrons
2. attraction of electrons for the positively charged nucleus
3. repulsive forces between neutrons
4. repulsive forces between protons
5. attraction of protons for neutrons
For the most common types of radioactive decay, the order of mass from lightest to heaviest is:
1. gamma, alpha, beta
2. beta, alpha, gamma
3. beta, gamma, alpha
4. gamma, beta, alpha
For the most common types of radioactive decay, the order of least penetrating to human tissue, to most penetrating to human tissue is:
1. gamma, alpha, beta
2. alpha, beta, gamma
3. beta, gamma, alpha
4. gamma, beta, alpha
If two electrons were removed from a calcium atom, the new particle is represented by:
1. Ca¹⁺
2. Ca²⁺
3. Ca^1-
4. Ca^2-
An atom or a group of atoms that has a net positive or negative charge is a(n):
1. isotope
2. molecule
3. ion
4. orbital
The energy change that occurs when an electron is acquired by a neutral atom is known as:
1. electron affinity
2. electronegativity
3. radioactivity
4. ionization energy
Generally speaking, the group of elements with the highest first ionization energy is:
1. Group 1
2. Group 16
3. Group 17
4. Group 18
Which of the following elements will have the greatest increase in ionization energy between the removal of the first and second electrons?
1. lithium
2. beryllium
3. boron
4. carbon
The most active metals are located in the:
1. lower right hand corner of the periodic table
2. lower left hand corner of the periodic table
3. upper right hand corner of the periodic table
4. upper left hand corner of the periodic table
Transition elements are classified as:
1. metals
2. nonmetals
3. metalliods
4. semiconductors
The current periodic table is organized:
1. by atomic weight order
2. alphabetically
3. by atomic number order
4. by mass number
Which of the following changes would result in the greatest shrinkage in atomic radius?
1. Gaining one electron to form a 1- anion
2. Gaining two electrons to form a 2- anion
3. Losing one electron to form a 1+ cation
4. Losing two electrons to form a 2+ cation
The least electronegative elements are the:
1. Noble gases
2. Alkali metals
3. Halogens
4. Metalloids
The metalloids possess properties of metals and nonmetals and are also known as:
1. gases
2. halogens
3. semimetals
4. liquids
The elements with the largest atomic radii are found in the:
1. upper right-hand corner of the periodic table
2. upper left-hand corner of the periodic table
3. lower right-hand corner of the periodic table
4. lower left-hand corner of the periodic table
The elements with the smallest atomic radii are found in the:
1. upper right-hand corner of the periodic table
2. upper left-hand corner of the periodic table
3. lower right-hand corner of the periodic table
4. lower left-hand corner of the periodic table
The measure of the attraction that an atom has for electrons involved in chemical bonds is known as:
1. electron affinity
2. electronegativity
3. radioactivity
4. ionization energy
The energy required to remove an electron from an atom is known as:
1. electron affinity
2. electronegativity
3. radioactivity
4. ionization energy
Given the representation of a chlorine atom, which circle might represent an atom of argon?
1. None of these
2. Circle B
3. Circle C
4. Circle D
Given the representation of a chlorine atom, which circle might represent an atom of sulfur?
1. None of these
2. Circle B
3. Circle C
4. Circle D
Given the representation of a chlorine atom, which circle might represent an atom of fluorine?
1. None of these
2. Circle B
3. Circle C
4. Circle D
Given the representation of a chlorine atom, which circle might represent an atom of bromine?
1. None of these
2. Circle B
3. Circle C
4. Circle D
Given the representation of a chlorine atom, which circle might a chloride ion, Cl^-?
1. None of these
2. Circle B
3. Circle C
4. Circle D
Which of the following elements is a halogen?
1. Iron(#26)
2. Germanium(#32)
3. Sulfur(#16)
4. Potassium(#19)
5. Iodine(#53)
Which of the following elements is a transition metal?
1. Iron(#26)
2. Germanium(#32)
3. Sulfur(#16)
4. Potassium(#19)
5. Iodine(#53)
Which of the following elements is a alkali metal?
1. Iron(#26)
2. Germanium(#32)
3. Sulfur(#16)
4. Potassium(#19)
5. Iodine(#53)
Which of the following elements is a semimetal?
1. Iron(#26)
2. Germanium(#32)
3. Sulfur(#16)
4. Potassium(#19)
5. Iodine(#53)
Which of the following elements is a nonmetal?
1. Iron(#26)
2. Germanium(#32)
3. Sulfur(#16)
4. Potassium(#19)
5. Iodine(#53)
Which of these elements is a halogen?
1. Element A
2. Element B
3. Element C
4. Element D
Which of these elements would have the lowest first ionization energy?
1. Element A
2. Element B
3. Element C
4. Element D
Element B is an:
1. alkali metal
2. alkaline earth metal
3. transition metal
4. halogen
Cations have a ______________ charge and are ______________ than the atoms from which they formed.
1. positive/larger
2. positive/smaller
3. negative/larger
4. negative/smaller
Anions have a ______________ charge and are ______________ than the atoms from which they formed.
1. positive/larger
2. positive/smaller
3. negative/larger
4. negative/smaller
High electronegativities are characteristic of:
1. nonmetals
2. metalloids
3. alkali metals
4. transition metals
Chemical bonds may be produced by any of the following processes involving electrons EXCEPT:
1. losing electrons
2. gaining electrons
3. splitting electrons
4. sharing electrons
The bond in between sodium and oxygen is expected to be:
1. ionic
2. nonpolar covalent
3. polar covalent
4. gaseous
The correct electron-dot notation for the element indium (atomic #49) is:
When compared to single bonds, double bonds are generally:
1. longer and stronger
2. shorter and weaker
3. shorter and stronger
4. longer and weaker
In the correct Lewis structure for water, how many unshared pairs of electrons will oxygen have?
1. 1
2. 2
3. 3
4. 4
Ionic compounds generally form:
1. molecules
2. crystals
3. liquids
4. gases
Which of the following is an acceptable Lewis Structure for the diatomic nitrogen molecule?
The seven elements that occur as diatomic elements are:
1. H₂, N₂, O₂, He₂, Ne₂, Cl₂, Br₂
2. H₂, N₂, O₂, He₂, Ne₂, C₂, Na₂
3. H₂, N₂, O₂, F₂, Cl₂, Br₂, I₂
4. Fe₂, Rn₂, O₂, He₂, Ne₂, C₂, Br₂
According to the HONC rule, how many covalent bonds form around hydrogen and the halogens?
1. one
2. two
3. three
4. four
Which of the following is an acceptable Lewis structure for chloromethane (CH₃Cl)?
According to the HONC rule, how many covalent bonds form around nitrogen?
1. one
2. two
3. three
4. four
The octet rule explains the stability of most covalently bonded molecules in terms of:
1. electronegativity differences
2. noble-gas configurations
3. ionization energies
4. electron affinities
In the correct Lewis structure for the methane (CH₄) molecule, how many unshared electron pairs surround the carbon?
1. 0
2. 2
3. 4
4. 8
In the sodium chloride crystal lattice, each positively charged ion is surrounded by how many ions of opposite charge?
1. 2
2. 4
3. 6
4. 8
In polar covalent bonds, valence electrons are:
1. transferred
2. equally shared
3. unequally shared
4. destroyed
In nonpolar covalent bonds, valence electrons are:
1. transferred
2. equally shared
3. unequally shared
4. destroyed
In ionic bonds, valence electrons are:
1. transferred
2. equally shared
3. unequally shared
4. destroyed
In a diatomic molecule of an element, the bond between the atoms must be:
1. ionic
2. polar covalent
3. nonpolar covalent
4. metallic
In metallic bonding, the valence electrons of all atoms are shared in:
1. a polar covalent bond
2. a nonpolar covalent bond
3. an electron sea
4. transferred to nonmetallic ions
The bond between lithium (atomic #3) and fluorine (atomic #9) is:
1. ionic
2. polar covalent
3. nonpolar covalent
4. metallic
How many sodium atoms are needed to provide the electrons necessary to complete the valence octet of an oxygen atom?
1. one sodium atom
2. two sodium atoms
3. three sodium atoms
4. four sodium atoms
In the ionic compound magnesium fluoride, what is the ratio of the two elements necessary so that each element obtains its octet from the transfer of electrons?
1. 1 magnesium : 1 fluorine
2. 2 magnesium : 1 fluorine
3. 1 magnesium : 2 fluorine
4. 3 magnesium : 1 fluorine
The amount of substance having the Avogadro number of any kind of chemical unit is called a(n):
1. atomic weight
2. mole
3. formula
4. mass number
The number of molecules in 18 grams of water is the same as that in how many grams of ammonia (NH₃)?
1. 17
2. 18
3. 30
4. 6.02x10²³
The formula mass of calcium hydroxide, Ca(OH)₂, is:
1. 57
2. 74
3. 97
4. 128
Three moles of sodium has a mass of approximately:
1. 23 grams
2. 69 amu
3. 69 grams
4. 1.8 x 10²⁴ grams
The sum of the average atomic masses of all the atoms present in the formula of any compound is called the:
1. formula mass
2. empirical masst
3. molecular mass
4. equation mass
About how many atoms of helium would be found in 2 grams of helium?
1. 6.02 x 10²³
2. 3.01 x 10²³
3. 2
4. 4.00260
According to the law of conservation of mass, the total mass of the reacting substances is:
1. always more than the total mass of products
2. always less than the total mass of products
3. always equal to the mass of the products
4. not related to the mass of the products
Which of the following gases does not exist in nature as a diatomic molecule?
1. helium
2. hydrogen
3. oxygen
4. nitrogen
When the synthesis reaction for iron(III) oxide
Fe + O₂ --> Fe₂O₃

is balanced, the coefficient on elemental iron is:
1. 1
2. 2
3. 3
4. 4

Isotope	Mass number	Atomic number	Protons	Neutrons	Electrons
Scandium-45