Hello please help
Which one of the following substances should exhibit hydrogen bonding in the liquid state?
NH3
PH3
H2
H2S
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How do chemical bonds form between the atoms in an ionic ompound?
sharing of atomic orbitals
sharing of all electrons
transfer of electrons from one atom to the other
sharing of valence electrons
Which is least likely to form an ion?
Li
Ar
F
Mg
Ionic compounds are good conductors of electricity when molten or aqueous.
False
True
In ionic compounds, __________ lose their valence electrons to form positively charged __________
nonmetals; anions
metals; cations
metals; polyatomic ions
metals; anions
What is the symbol for the ion with 19 protons and 18 electrons?
K+
Ar
F-
F+
Transition metals form 2 or more positive ions.
True
False
No answer text provided.
Which of the following are properties of ionic compounds?
high boiling point
conductor of electricity
gas at room temperature
high metling point
You observe that a compound is hard and brittle, smells salty, dissolves in water, and conducts electricity. You conclude that the compound more likely is a(n)...
ionic compound
a sugar
SO2
covalent compound
Which two elements would NOT be capable of forming an ionic bond?
calcium and oxygen
barium and nitrogen
oxygen and chlorine
sodium and chlorine
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Melting points of ionic compounds tend to be _____.
very high
very low
slightly above room temperature
ower than those of molecular compounds
Will solid NaCl conduct electricity?
No
Yes
Double and triple bonds form because
the atoms involved have high electronegativities.
one of the atoms in the molecule has more than eight valence electrons.
there is at least one hydrogen atom involved in the bond.
single covalent bonds do not give all of the atoms in the molecule eight valence electrons.
A triple bond involves the sharing of ________ pairs of electron(s) between the atoms.
2
3
4
6
The sharing of 4 electrons between atoms forms a(n)...
unstable bond
triple bond
double bond
single bond
Which of the following molecules forms a double bond?
O2
Cl2
CH4
N2
Which property is most closely associated with covalent molecules?
It is composed of a metal and a nonmetal.
It has a very high melting point.
It is composed of a two metals.
It is a gas at room temperature.
Which of the following compounds contains only bonds in which electrons are shared?
CuNO3
LiOH
PCl3
BaS
Which factor distinguishes a metallic bond from an ionic bond or a covalent bond?
Unequal sharing of core electrons
Electron transfer from one atom to another
Equal sharing of electrons
Dissociation of valence electrons
How do chemical bonds form between the atoms in a covalent compound?
exchange of atomic orbitals
transfer of electrons from one atom to the other
sharing of valence electrons
sharing of all electron
In which of the following compounds is the bond between the two atoms most likely a nonpolar covalent bond?
HCl
H2O
NH3
H2
What will be the molecular geometry with three electron domain around the central atom with no lone pair?
Trigonal pyramidal
Tetrahedral
Trigonal planar
Linear
Which diatomic molecule is doubly bound (has a double bond)?
Cl2
O2
H2
N2
Which of the following molecule is most likely polar?
BeF2
CO2
CCl4
NCl3
Which of the following molecules is most likely nonpolar?
H2O
SO2
CH4
NH3
Which intermolecular force(s) is responsible for the interactions between molecules of PH3?
Both London dispersion forces and hydrogen bonds
Dipole-dipole forces
London dispersion forces
Hydrogen bonds
Which substance involves no intermolecular forces except London dispersion forces?
H2O
NH3
N2
HF
For which of the following species are the dispersion forces strongest?
C7H16
C6H14
C8H18
C4H10
Which of the following atoms does not participate in hydrogen bonding?
F
S
N
O
Order the intermolecular forces (dipole-dipole, London dispersion, ionic, and hydrogen-bonding) from weakest to strongest .
hydrogen-bonding, dipole-dipole, London dispersion, and ionic
dipole-dipole, London dispersion, ionic, and hydrogen-bonding
London dispersion, dipole-dipole, hydrogen-bonding, and ionic
dipole-dipole, ionic, London dispersion, and hydrogen-bonding
Atoms having equal or nearly equal electro negativities are expected to form
nonpolar covalent bonds
ionic bonds
no bonds
polar covalent bonds
