An ion is defined as a ____________
a. Charged atom that has gained or lost electrons
b. Atom that has gain an single electron
c. Metal that has become charged
d. A neutral atom formed after bonding has occurred
a. Charged atom that has gained or lost electrons
100
Which one of the following is an example of a diatomic molecule?
a. H2O
b. KF
c. H2
d. H2SO4
c. H2
100
The electrons in the outer most shell of an atom are the ______________
a. Oxidation electrons
b. Lone pair electrons
c. Valence electrons
d. Ionic electrons
c. Valence electrons
100
The charge on an ion that forms as electrons are gained or lost is indicated by the _______.
a. Oxidation number
b. Electronegativity value
c. Cation
d. Valence electrons
a. Oxidation number
100
A bond that forms when electrons are unequally shared between two atoms is a ________
a. Ionic bond
b. Non-polar covalent bond
c. Polar covalent bond
d. Pure non-polar covalent bond
c. Polar covalent bond
200
A bond that forms as electrons are transferred from a positive ion to a negative ion is a _________
a. Covalent bond
b. Ionic bond
c. Metallic bond
d. Triple bond
b. Ionic bond
200
A bond that forms when electrons are shared within the bond is a ___________
a. Ionic bond
b. Covalent bond
c. Polyatomic bond
d. Metallic Bond
b. Covalent bond
200
The change of electrons in Pb2+ is
a. one electron lost
b. one electron gained
c. two electrons lost
d. two electrons gained
c. two electrons lost
200
A positive ion forms when ________
a. An atom gains electrons
b. An atom loses electrons
c. An atom shared electrons
d. An atom bonds with itself
b. An atom loses electrons
200
All atoms bond to reach a stable formation of ________ electrons.
a. 8
b. 4
c. 2
d. 10
a. 8
300
Which one the following is NOT a property of a solid formed from an ionic bond?
a. Form hard, brittle solids
b. Malleability
c. High boiling point
d. Form repeating crystalline patterns
b. Malleability
300
Which of the following is NOT a property caused by covalent bonding?
a. Low melting and boiling points
b. Non-conductive
c. Form repeating crystal structures
d. Form soft solids
c. Form repeating crystal structures
300
Sn(IV) is the symbol for
a. Tin -4
b. Antimony -4
c. Tin +4
d. Sodium +4
c. Tin +4
300
In an ionic formula, what does a Roman numeral indicate?
a. The charge on the cation
b. The number of valence electrons the ion has
c. The ratio of cations to anions
d. The number of each atoms in the compound
a. The charge on the cation
300
Electronegativity is defined as __________
a. The amount of energy needed to remove an electron in a chemical bond
b. The geometric shape of a molecule
c. The tendency of an atom to pull electrons to itself in a chemical bond
d. The tendency of an atom to lose electrons when forming bonds
c. The tendency of an atom to pull electrons to itself in a chemical bond
400
What is the correct name for Fe(OH)2?
a. Ferric hydroxide
b. Ferrous hydroxide
c. Iron (II) peroxide
d. Iron (II) hydroxide
b. Ferrous hydroxide
or
d. Iron (II) hydroxide
400
All covalent bonds will contain _____ pairs of electrons
a. 10
b. 2
c. 4
d. 1
d. 1
400
Electrons have a ________ charge and can be found in the _________ of an atom.
a. Negative, nucleus
b. Negative, cloud
c. Positive, cloud
d. Neutral, nucleus
b. Negative, cloud
400
A negatively charged ion is also called a(n) __________
a. Cation
b. Alloy
c. Polyatomic ion
d. Anion
d. Anion
400
Which of the following would be an example of a polar molecule?
a. O2
b. NaCl
c. CH4
d. H2O
d. H2O
500
The correct formula for calcium carbonate is
a. CaCO
b. Ca3CO
c. CaCO3
d. Ca(CO3)2
c. CaCO3
500
What is the formula for carbon tetrabromide?
a. CBr3
b. CBr4
c. CaBr4
d. CaBR4
b. CBr4
500
How many electrons are in each of the first 4 energy levels?
a. 2, 4, 6, 8
b. 2, 8, 14, 36
c. 2, 8, 18, 32
d. 2, 14, 27, 64
c. 2, 8, 18, 32
500
What is the correct oxidation state for Ge?
a. +3
b. -3
c. +4
d. -4
c. +4
500
A bond that forms from the attraction between a metal cation and the delocalized electrons is a __________ bond
a. Ionic
b. Metallic
c. Covalent
d. Polar