WorksheetsExam 1 Study Set
Total questions: 60
Worksheet time: 32mins
What is deposition?
Liquid to gas
Solid to liquid
Solid directly to gas
Gas directly to solid
What is sublimation?
Liquid to gas
Solid to liquid
Solid directly to gas
Gas directly to solid
What produces when you heat a liquid in a closed container until its temperature is beyond the critical temperature?
Supercritical fluid
Gas
Solid
Liquid
(a) is the transition from solid to liquid
Fusion is exothermic
True
False
Enthalpy of vaporization generally decreases with increasing strength of intermolecular forces
True
False
The critical point has a temperature of...
140 °C
125 °C
76 °C
80 °C
What state of matter is the following substance in at room temperature and standard pressure
Solid
Liquid
Gas
Supercritical fluid
All 3 states of matter can exist at equilibrium at what temperature and pressure?
76 °C and 0.56 atm
125 °C and 1.0 atm
140 °C and 2.37 atm
80 °C and 1.0 atm
The normal boiling point of the substance is...
76 °C
80 °C
125 °C
140 °C
Identify the type of solid for AgCl (hint: Ag has a 1 valence electron)
Ionic solid
Covalent solid
Metallic solid
Nonbonding solid
Network covalent solids generally have high melting points, and are held together by covalent bonds
True
False
Nonbonding atomic solids are held together by dipole-dipole forces.
True
False
Which intermolecular force is experienced by all molecules?
London dispersion forces
Dipole-dipole forces
Hydrogen bonding
Ion-dipole forces
Hydrogen bonding can only occur when hydrogen bonds with which element(s)?
Hydrogen
Bromine and Barium
Nitrogen, Oxygen, or Fluorine
Carbon, Nitrogen, or Fluorine
Which intermolecular force is the strongest in a pure substance
London dispersion forces
Dipole-dipole forces
Hydrogen bonding
Ion-dipole forces
Which of these would exhibit Ion-dipole forces?
NaBr(aq)
KCL(aq)
H20(aq)
C4H10
As the mass of a compound increases the dispersion forces between the bonds does what?
Remains the same
Gets stronger
Gets weaker
Doesn't exist
intermolecular forces are _______ bonds
Weaker than
Stronger than
Equal in strength to
The same as
What is the strongest intermolecular force present in H2CO
London dispersion forces
Dipole-dipole forces
Hydrogen bonding
Ion-dipole forces
What is the strongest intermolecular force present in CH3COOH?
Dispersion forces
Dipole-dipole forces
Hydrogen bonding
Ion-dipole forces
What is the strongest intermolecular force present in SiF4?
Dispersion forces
Dipole-dipole forces
Hydrogen bonding
Ion-dipole forces
What is the strongest intermolecular force present in C4H10
Dispersion forces
Dipole-dipole forces
Hydrogen bonding
Ion-dipole forces
What is the strongest intermolecular force present in NH3?
Dispersion forces
Dipole-dipole forces
Hydrogen bonding
Ion-dipole forces
You can change from a liquid to a gas by increasing temperature or decreasing pressure
True
False
You can change from gas to a liquid by decreasing temperature or increasing pressure?
True
False
Solids can be categorized as crystalline or amorphous; crystalline solids have long-range order
True
False
In a liquid, the particles can move with respect to one another, so liquids have a definite shape, but indefinite volume.
True
False
What is condensation?
Gas to liquid
Liquid to gas
Solid to liquid
Liquid to solid
The boiling point of a liquid is when the vapor pressure of the liquid is equal to the external pressure
True
False
The rate of vaporization decreases with increasing temperature and surface area, but increasing intermolecular forces.
True
False
Dynamic equilibrium is reached when the condensation and vaporization processes stop
True
False
If you bring a pot of water from sea level to La Paz, Bolivia (11,975 ft above sea level), you will decrease its boiling point
True
False
Molecular solids generally have low melting points and the repeating unit in the crystal structure in the molecule; an example is dry ice
True
False
Network covalent solids generally have high melting points and are held together by covalent bonds; an example is graphite
True
False
Iron (II) oxide is an example of an atomic crystalline solid; it is held together by metallic bonds.
True
False
Nonbonding atomic solids are held together by dispersion forces and generally have low melting points; an example is N2
True
False
Ionic solids generally have high melting points and are held together by electrostatic interactions; an example is barium chloride
True
False
H2CO has a lower melting point than CH3OH
True
False
A nonpolar solvent like CCl4 should be used to dissolve KCl
True
False
C6H14 should have a lower boiling point than C7H16
True
False
A polar solvent like H2O should be used to dissolve H2CO
True
False
What is the molecular geometry of NH3
Trigonal planar
Trigonal pyramidal
Linear
Tetrahedral
Indicate the molecular geometry for PF3
Trigonal pyramidal
Bent
Trigonal planar
linear
Indicate the molecular geometry for CO2
Trigonal pyramidal
Trigonal planar
Linear
Bent
Indicate the geometry of BrF3
Tetrahedral
T-shape
Seesaw
Trigonal planar
When a solution forms, the solute-solute interactions must be overcome, so ΔHsolute is exothermic
True
False
It is possible to have a solution where the solvent and solute are both in the gas phase
True
False
The spontaneous mixing of two ideal gases when a barrier is removed is an example of an increase in entropy
True
False
If the solvent-solute interactions are stronger than the solvent-solvent and solute-solute interactions, a solution will generally form
True
False
Solubility of most solids increases with increasing temperature
True
False
Solubility of most gases increases with increasing pressure and decreasing temperature
True
False
A solution that contains more dissolved solute than the equilibrium amount is saturated
True
False
A solution in which the dissolved solute is in dynamic equilibrium with the solid (undissolved) solute is a supersaturated solution
True
False
Which are polar?
XeF2
BrF3
CH3OCH3
C4H10
What pressure of He is required to maintain the He concentration in a bottle at 0.1 M? Henry's Law constant for He is 3.7 x 10-4 M/atm. 3 significant figures
(a)
What is Molarity (M)
amount solute (in mol)/volume solution in (L)
amount solute (in mol)/mass solvent (in kg)
(amount solute (in mol)/total amount of solute and solvent (in mol)) x 100%
(mass solute/mass solution) x 100
What is molality (m)
amount solute (in mol)/volume solution (in L)
amount solute (in mol)/mass solvent (in kg)
amount solute (in mol)/total amount of solute and solvent (in mol)
(mass solute/mass solution) x 100
What is mole fraction (χ)
amount solute (in mol)/volume solution (in L)
amount solute (in mol)/mass solvent (in kg)
amount solute (in mol)/total amount of solute and solvent (in mol)
(mass solute/mass solution) X 100
What is percent by mass (%)
amount solute (in mol)/volume solution (in L)
amount solute (in mol)/mass solvent (in kg)
amount solute (in mol)/total amount of solute and solvent (in mol)
(mass solute/mass solution) X 100 %
