Test Bank for General Chemistry 1and 2
The Essential Concept 7th Edition by
Raymond Chang 2024 (Graded A+)
What happens to the boiling point when the external pressure on a liquid increases? -
ANS-The boiling point increases
What happens at the critical point in a phase diagram? - ANS-At the critical point, the
densities of the liquid and gas phases become equal.
What happens at the triple point in a phase diagram? - ANS-At the triple point, all three
phases are in equilibrium.
more polarizable = stronger .... .... - ANS-intermolecular force
What are the trends in polarizability? - ANS-Polarizability decreases across a period
because of increasing Zeff.
Polarizability increases down a group because atomic size increases and larger
electron clouds distort more easily.
In general, smaller particles are less polarizable than larger ones because their
electrons are held more tightly.
When do dispersion or london forces arise? - ANS-When an instantaneous dipole in
one particle induces a dipole in another, resulting in an attraction between them.
Memorize figure 12.19 (summary diagram) - ANS-If there are interacting particles then
they are separated into 2 categories.
For ions present, if there are ions only, it is ionic bonding. If there are ions and polar
molecules, it is ion-dipole forces.
When there are no ions present, for polar molecules, it could be dipole-dipole, unless
hydrogen is bonded to n, o, or f, which means it'd be hydrogen bonding. Another section
is the polar & nonpolar molecules, which would be dipole-induced dipole forces. The
final one would be nonpolar with only dispersion forces.
molarity equation - ANS-amount (mol) of solute/ volume (L) of solution
parts by volume equation - ANS-volume of solute/volume of solution
molality equation - ANS-amount(mol) of solute/mass (kg) of solvent
parts by mass equation - ANS-mass of solute/mass of solution
, mole fraction equation - ANS-amount(mol) of solute/amount of solute +amount of
solvent
The stronger the forces between the particles the higher the .... ..... - ANS-surface
tension
Dispersion forces are stronger for which type of particles? - ANS-larger, more
polarizable particles
Which two things affect viscosity? - ANS-1) Increasing temperature decreases viscosity
2) Given the same types of intermolecular forces, liquids consisting of longer molecules
have higher viscosities.
When the strength of the intermolecular forces increase, what happens to vapor
pressure? - ANS-It decreases
Bonding forces are stronger than nonbonding (intermolecular) forces.
Hydrogen bonding is a strong type of dipole-dipole force.
Dispersion forces are decisive when the difference is molar mass or molecular shape. -
ANS-Bonding forces are stronger than nonbonding (intermolecular) forces.
Hydrogen bonding is a strong type of dipole-dipole force.
Dispersion forces are decisive when the difference is molar mass or molecular shape.
Solids are divided into 2 categories: - ANS-crystalline solids & amorphous solids
How many atoms are there in a simple cubic unit cell? - ANS-1
How many atoms are there in a body-centered cubic unit cell? - ANS-2
How many atoms are there in a face-centered cubic unit cell? - ANS-4
In atomic solids, which type of interparticle forces are possible? - ANS-dispersion
In molecular solids, which type of interparticle forces are possible? - ANS-dispersion,
dipole-dipole or h bonds
In ionic solids, which type of interparticle forces are possible? - ANS-ion-ion attraction
In metallic solids, which type of interparticle forces are possible? - ANS-metallic bonds
In network covalent solids, which type of interparticle forces are possible? - ANS-
covalent bonds
What happens to vapor pressure as temperature increases? - ANS-Vapor pressure
increases
The Essential Concept 7th Edition by
Raymond Chang 2024 (Graded A+)
What happens to the boiling point when the external pressure on a liquid increases? -
ANS-The boiling point increases
What happens at the critical point in a phase diagram? - ANS-At the critical point, the
densities of the liquid and gas phases become equal.
What happens at the triple point in a phase diagram? - ANS-At the triple point, all three
phases are in equilibrium.
more polarizable = stronger .... .... - ANS-intermolecular force
What are the trends in polarizability? - ANS-Polarizability decreases across a period
because of increasing Zeff.
Polarizability increases down a group because atomic size increases and larger
electron clouds distort more easily.
In general, smaller particles are less polarizable than larger ones because their
electrons are held more tightly.
When do dispersion or london forces arise? - ANS-When an instantaneous dipole in
one particle induces a dipole in another, resulting in an attraction between them.
Memorize figure 12.19 (summary diagram) - ANS-If there are interacting particles then
they are separated into 2 categories.
For ions present, if there are ions only, it is ionic bonding. If there are ions and polar
molecules, it is ion-dipole forces.
When there are no ions present, for polar molecules, it could be dipole-dipole, unless
hydrogen is bonded to n, o, or f, which means it'd be hydrogen bonding. Another section
is the polar & nonpolar molecules, which would be dipole-induced dipole forces. The
final one would be nonpolar with only dispersion forces.
molarity equation - ANS-amount (mol) of solute/ volume (L) of solution
parts by volume equation - ANS-volume of solute/volume of solution
molality equation - ANS-amount(mol) of solute/mass (kg) of solvent
parts by mass equation - ANS-mass of solute/mass of solution
, mole fraction equation - ANS-amount(mol) of solute/amount of solute +amount of
solvent
The stronger the forces between the particles the higher the .... ..... - ANS-surface
tension
Dispersion forces are stronger for which type of particles? - ANS-larger, more
polarizable particles
Which two things affect viscosity? - ANS-1) Increasing temperature decreases viscosity
2) Given the same types of intermolecular forces, liquids consisting of longer molecules
have higher viscosities.
When the strength of the intermolecular forces increase, what happens to vapor
pressure? - ANS-It decreases
Bonding forces are stronger than nonbonding (intermolecular) forces.
Hydrogen bonding is a strong type of dipole-dipole force.
Dispersion forces are decisive when the difference is molar mass or molecular shape. -
ANS-Bonding forces are stronger than nonbonding (intermolecular) forces.
Hydrogen bonding is a strong type of dipole-dipole force.
Dispersion forces are decisive when the difference is molar mass or molecular shape.
Solids are divided into 2 categories: - ANS-crystalline solids & amorphous solids
How many atoms are there in a simple cubic unit cell? - ANS-1
How many atoms are there in a body-centered cubic unit cell? - ANS-2
How many atoms are there in a face-centered cubic unit cell? - ANS-4
In atomic solids, which type of interparticle forces are possible? - ANS-dispersion
In molecular solids, which type of interparticle forces are possible? - ANS-dispersion,
dipole-dipole or h bonds
In ionic solids, which type of interparticle forces are possible? - ANS-ion-ion attraction
In metallic solids, which type of interparticle forces are possible? - ANS-metallic bonds
In network covalent solids, which type of interparticle forces are possible? - ANS-
covalent bonds
What happens to vapor pressure as temperature increases? - ANS-Vapor pressure
increases
