Transcript Chapter 10 Review States of Matter
Chapter 9 - Review States of Matter
Chapter 9 - Review
• What happens to the range of energies of the molecules in matter when the temperature is increased?
• What happens to the average kinetic energy of the particles in a sample of matter as the temperature is increased?
Chapter 9 - Review
• Consider an iron ball and an aluminum ball. If the two balls were at the same temperature, how would their average kinetic energies compare?
• Which temperature scale provides a direct measure of the average kinetic energy of a substance?
Chapter 9 - Review
• What instrument is normally used to measure atmospheric pressure?
• What is the SI unit of pressure?
• How does the atmospheric pressure at altitudes below sea level compare with atmospheric pressure at sea level?
Chapter 9 - Review
• What volume does 3.00 moles of gas particles occupy at STP?
• What is the volume occupied by 2.20 mol of hydrogen at STP • What is the number of moles of gas in 20.0 L of oxygen at STP • What is the number of molecules of nitrogen in 11.2 L at STP?
Chapter 9 - Review
• What is the volume occupied by 14.0 x 10
23
molecules of fluorine at STP?
• What is the volume occupied by 71.0 g of chlorine gas at STP?
• What is the number of grams of neon present in 78.4 L of neon at STP?
Chapter 9 - Review
• How many iron molecules are moving in a piece of steel?
• Collisions between gas molecules are ____.
• The average speed of oxygen molecules in air is approximately ___.
Chapter 9 - Review
• How far can a molecule travel in air before it collides with another molecule?
• Which would have the greatest kinetic energy: steam at 200
o
C, or water at 373 K • Describe the kinetic theory of gases.
Chapter 9 - Review
• What happens when a gas is heated?
• The average kinetic energy of the particles of a substance is proportional to the ____ of the substance.
• The temperature at which the motion of particles theoretically ceases is ____
Chapter 9 - Review
• What is the pressure of one standard atmosphere?
• Standard conditions when working with gases are defined as ____.
• The pressure of a gas in a container is 152 mm Hg. This is equivalent to _____ atm.
Chapter 9 - Review
• Compared with 1 mole of chlorine gas at STP, what volume would 1 mole of hydrogen gas at STP occupy?
• It is possible for equal volumes of gases, at the same temperature and pressure, to contain equal numbers of particles because ___.
Chapter 9 - Review
• Equal volumes of nitrogen and oxygen, at the same temperature and pressure, would contain ____ numbers of particles.
• Which states of matter can flow?
• What happens to the temperature of a liquid as it evaporates?
Chapter 9 - Review
• What happens to the evaporation rate of a liquid as the liquid is cooled?
• Why does a liquid’s evaporation rate increase when the liquid is heated?
• When the external pressure is 505 kPa, what is the vapor pressure of water at it’s boiling point?
Chapter 9 - Review
• If heat is added to a boiling liquid, what happens to the temperature of the liquid?
• What types of forces exist between particles of a liquid?
• What are the condensed states of matter?
Chapter 9 - Review
• The first particles to evaporate from a liquid are ____.
• Which of the following will evaporate fastest: water at 20
o
C, or water at 40
o
C?
• If a liquid is sealed in a container and kept at constant temperature, how does it’s vapor pressure change over time?
Chapter 9 - Review
• In a dynamic equilibrium between the liquid state and the gas state, the rate of evaporation is ____.
• An increase in the temperature of a contained liquid causes the vapor pressure above the liquid to ___.
• The escape of gas molecules from the surface of an uncontained liquid is known as ______.
Chapter 9 - Review
• What is the pressure when a liquid is boiling at it’s normal boiling point?
• When the vapor pressure of a liquid is equal to atmospheric pressure, the liquid ____.
• Water could be made to boil at 105
o
C instead of 100
o
C by ___.
Chapter 9 - Review
• Crystals are classified into how many different crystal systems?
• The boiling points of ionic solids tend to be ____.
• Crystals are characterized by particular patterns that repeat ___.
• Different crystal systems differ in the _____.
Chapter 9 - Review
• The repeating group of a crystal is called the ___.
• Which of the following forms of carbon is an amorphous solid: graphite, diamond, or soot?
• Glasses are sometimes called ____ liquids.
Chapter 9 - Review
• Most solids are ___ and _____.
• Which of the following elements is characterized by it’s ability to undergo sublimation: iodine, carbon, sodium, or oxygen?
• Which of the following is NOT a phase change: melting, diffusion, sublimation, or vaporization?
Chapter 9 - Review
• The direct change of a substance from a solid to a gas is called ____.
Chapter 10 – Review The Behavior of Gases
Chapter 10 - Review
• Know the assumptions of the kinetic theory.
• Why does the pressure inside a container of gas increase if more gas is added to the container?
• Why does air leave a tire when the tire valve is opened?
Chapter 10 - Review
• If 4 moles of gas are added to a container that already holds 1 mole of gas, how will the pressure change within the container?
• Increasing the volume of a given amount of gas at constant temp. causes the pressure to decrease because _______.
Chapter 10 - Review
• If the volume of a container holding a gas is reduced, what will happen to the pressure within the container?
• What happens to the temperature of a gas when it is compressed?
Chapter 10 - Review
• What happens to the pressure of a gas inside a container, if the temperature of the gas is lowered?
• If a balloon is squeezed, what happens to the air pressure within the balloon?
Chapter 10 - Review
• The volume of a gas is doubled while the temperature is held constant. How does the gas pressure change?
• The volume of a gas is reduced from 4.0 L to 0.5 L while the temperature is held constant. How does the gas pressure change?
Chapter 10 - Review
• A gas occupies a volume of 0.7 L at 10.1
o
kPa. What volume will the gas occupy at 101 kPa?
• A sample of gas occupies 40 mL at –123 C. What volume does the sample occupy at 27
o
C?
• What type of changes could cause an increase in the pressure of a gaseous system?
Chapter 10 - Review
• Why does an aerosol can become cooler when gas is released?
• As the temperature of a fixed volume of gas increases, the pressure will _____.
• As the temperature of a balloon decreases, the average kinetic energy _____.
Chapter 10 - Review
• Boyle’s law states that _____.
• When the temperature and number of particles are kept constant for a sample of gas, what is also constant for the sample?
• Charles’ law states that _____.
Chapter 10 - Review
• If a balloon is rubbed vigorously, what happens to the volume of the air in the balloon if the pressure is held constant?
• When the pressure and number of particles are kept constant for a gas, what else is kept constant?
Chapter 10 - Review
• If a capped syringe is plunged into cold water, in which direction will the syringe piston slide?
• If a balloon is rubbed vigorously, what happens to the pressure of the air inside the balloon if the volume remains constant?
Chapter 10 - Review
• Generally, for a gas at a constant volume, the pressure is _____ proportional to its temperature in Kelvin.
• If a capped syringe is heated, in which direction will the syringe piston move?
• The combined gas law relates to what variables?
o
is 10
o
Chapter 10 - Review
• If a balloon containing 1000 L of gas at 50 C and 101 kPa rises to an altitude where the pressure is 50.5 kPa and the temperature C, the volume of the balloon under these new conditions would be _____.
Chapter 10 - Review
• At very high pressures, how does the volume of a real gas compare with the volume that would be predicted for an ideal gas under the same conditions?
• At low temp. and pressure, how does the volume of a real gas compare with an ideal gas?
____.
PV/T
Chapter 10 - Review
• An ideal gas CANNOT be converted to a • When the volume and number of particles are held constant for a sample of gas, what else is kept constant?
• Which is constant for 1 mole? PT/V or
Chapter 10 - Review
• What does the ideal gas law allow a scientist to calculate that the other laws do not?
• What is the normal form of the ideal gas law equation?
Chapter 10 - Review
• At a certain temperature and pressure, 0.20 mol of CO molecules.
2
has a volume of 3.1 L. A 3.1 L sample of hydrogen at the same temperature and pressure contains ______ • Under what conditions is the behavior of a real gas like that of an ideal gas?
Chapter 10 - Review
• If oxygen is removed from the air in the process of rusting, what happens to the partial pressure of oxygen in the air?
• If oxygen is removed from the air in the process of rusting, what happens to the total pressure of the air?
Chapter 10 - Review
• What happens to the partial pressure of oxygen in the air if the air temperature is increased?
• If the volume of a container of air is reduced by one-half, what happens to the partial pressure of oxygen within the container?
Chapter 10 - Review
• A breathing mixture used by deep-sea divers contains helium, oxygen, and carbon dioxide. What is the partial pressure of oxygen at 101 kPa, if P
He
= 84 kPa and P
CO2
= 0.1 kPa?
Chapter 10 - Review
• When a container is filled with 3 moles of H
2
, 2 moles of O
2
, and 1 mole of N
2
, the pressure in the container is 8787 kPa. What is the partial pressure of O
2
?
Chapter 10 - Review
• If the atmospheric pressure on Mt. Everest is one-third the atmospheric pressure at sea level, the partial pressure of oxygen on Mt. Everest is _____.
• The tendency of molecules to move toward areas of lower concentration is called _____.
Chapter 10 - Review
• A box with a volume of 22.4 L contains 1.0 mol of nitrogen and 2.0 moles of hydrogen at 0
o
C. What is the partial pressure of the nitrogen?
• Which gas would effuse most rapidly: chlorine or hydrogen?
Chapter 10 - Review
• Which of the following atoms would have the greatest velocity if each atom had the same kinetic energy: hydrogen or bromine?
Chapter 10 - Review
• Which of the following gases is the best choice to serve as the inflating gas of a balloon that must remain inflated for a long period of time: hydrogen or argon?
Chapter 5 - Review Chemical Names and Formulas
Chapter 5 Review
• What type of ions have names ending in ide?
• What is the electrical charge of a cation?
• Give the charge and number of electrons for the calcium ion.
• How many electrons in Sr
2+
; Kr; Br
1-
?
Chapter 5 Review
• How are cations formed?
• Ions form when atoms gain or lose _____.
• Which is a pure compound: fresh air; salt water; calcium iodide?
• In any chemical compound, the elements are always combined in the same proportion by ____.
Chapter 5 Review
• The Law of Definite Proportions applies to what type of materials?
• Know the properties of molecular compounds.
• What are ionic compounds composed of?
Chapter 5 Review
• What is the lowest whole-number ratio of ions in an ionic compound called?
• Which of the following formulas represents an ionic compound: Kr; BaI
2
; N
2
O
4
• Which represents a molecular compound: Xe; ZnO; SO
2
Chapter 5 Review
• What are molecular compounds usually composed of?
• Which element when combined with fluorine would most likely form an ionic compound: phosphorus; lithium; chlorine • Ionic compounds have relatively _____ melting and boiling points.
Chapter 5 Review
• What information is obtained about the formula C
2
H
6
O?
• What is the charge on a formula such as K
2
O?
• Ionic compounds are composed of ____ and ____ ions.
• What information does a molecular formula give?
Chapter 5 Review
• Which of the following pairs of substances best illustrates the Law of Multiple Proportions: NO and NO
2
; P
2
O
5
and PH
3
• What is the usual charge on an ion from Group 7A?
• What is the charge on an ion of: potassium; strontium; oxygen
Chapter 5 Review
• Give the name for the following ions: Fe
2+
and Fe
3+
• What is the charge on an ion of: calcium; aluminum; bromine • How does an element from Group 2 form ions?
• Give the name and symbol for an ion of: copper (I); fluorine
Chapter 5 Review
• What type of ions are commonly formed from Group 4A elements?
• How do the metals in Groups 1A, 2A, and 3A form ions?
• Name the following: OH
1-
; O
2-
• Polyatomic ions are tightly bound groups of _____.
Chapter 5 Review
• Name: CrO
4 2-
and Cr
2
O
7 2-
• An -ate or -ite at the end of a compound name usually indicates that the compound contains ___.
• What is the ionic charge on the zirconium ion in the ionic compound zirconium oxide, ZrO
2
?
Chapter 5 Review
• What is the correct name for the N
3-
ion?
• What is the correct formula for potassium sulfite?
• What is the correct formula for barium chlorate?
• Ternary ionic compounds contain three different ______.
Chapter 5 Review
• What is the correct formula for calcium dihydrogen phosphate?
• Why are systematic names preferred over common names?
• What compound is formed by combining Au
3+
and S
2-
?
Chapter 5 Review
• What is the ionic charge on the thorium ion in ThO
2
?
• What is the formula of the ionic compound from combining Sc
3+
and S
2-
?
Chapter 5 Review
• Name SnF
4
and Na
2
O.
• Which of the following contains the lead (IV) ion: Pb
4
O
3
; Pb
2
O; PbO
2
• Which contains the Mn
3+
ion: Mn
2
O
3
Mn
3
O
2
or
Chapter 5 Review
• The procedure for writing formulas for ternary ionic compounds is the same as that for binary ionic compounds, with the exception that _______.
Chapter 6 Review
“The Periodic Table”
Chapter 6 Review
• Which of the following groupings contains only representative elements: a) Cu, Co, Cd, or b) Al, Mg, Li?
• What is true about the electron configurations of the representative elements?
• The metals in Groups 1A, 2A, and 3A ___ electrons when forming ions.
Chapter 6 Review
• What are the Group 1A and Group 7A elements examples of?
• Which of the following elements has the smallest radius: a) chlorine, or b) bromine?
• How does the size of an ion compare to the atom it came from?
• The modern periodic table is arranged according to _____.
Chapter 6 Review
• In which of the following groups of ions are the charges all shown correctly: a) Li
1-
, O
2-
, S
2+
, or b) Ca
2+
, Al
3+
, Br
1-
?
• Which of the following elements are nonmetal: Pt, V, Li, and Kr • Know the characteristics of cations and anions.
Chapter 6 Review
• What is another name for the transition metals?
• Which of the following elements is a transition metal: a) copper, or b) cesium?
• What is the factor that contributes to the increase in ionization energy from left to right across a period?
Chapter 6 Review
• To what category of elements does an element belong if it is a poor conductor of electricity?
• What is the charge of a cation?
• Which of these elements has the lowest electronegativity value: a) cesium, or b) calcium?
• Which of the following is correct: a) In, 49 protons, 49 electrons, or b) Zn, 30 protons, 60 electrons?
Chapter 6 Review
• What element in the second period has the largest atomic radius?
• Which of the following elements is in the same period as phosphorus: a) magnesium, or b) nitrogen?
• Who arranged the elements according to atomic mass, and used the arrangement to predict the properties of missing elements?
Chapter 6 Review
• What causes the shielding effect to remain constant across a period?
• For Group 2A metals, which electron is the most difficult to remove?
• What is true about the electron configurations of the noble gases?
• What category includes the majority of the elements?
Chapter 6 Review
• What is the element with the highest electronegativity value: a) calcium, or b) fluorine?
• Which subatomic particle plays the greatest part in determining the properties of an element?
• Of the following, which one has the smallest first ionization energy: a) aluminum, or b) silicon?
Chapter 6 Review
• What element has the electron configuration of 1s
2
2s
2
2p
6
3s
2
3p
2
?
• In which of the following sets are the charges given correctly for all the ions: a) Na
1+
, Mg
1+
, Al
1+
, or b) K
1+
, Sr
2+
, O
2-
?
• Which of the following elements has the smallest ionic radius: a) Li, or b) K?
Chapter 6 Review
• What electron configuration is most likely to result in an element that is relatively inactive?
• How does atomic radius change from left to right across a period in the periodic table?
• How does atomic radius change from top to bottom in a group in the periodic table?
Chapter 6 Review
• Elements that are characterized by the filling of p orbitals are classified as _____.
• As you move from left to right across the second period of the periodic table, ionization energy __.
• Atomic size generally decreases as you ____.
Chapter 6 Review
• Which of the following is a representative element: a) Fe, or b) Te • Cations form when an atom ____ electrons.
• What is the energy required to remove an electron from an atom in the gaseous state called?
Chapter 6 Review
• Which of the following decreases with increasing atomic number in Group 2A: a) ionization energy, or b) ionic size?
• What is another name for the representative elements?
• Each period in the periodic table corresponds to ____.
Chapter 6 Review
• Which of the following elements has the smallest first ionization energy: a) potassium, or b) magnesium?
• Compared with the electronegativity of elements on the left side of a period, the electronegativity of the elements on the right side of the same period tend to be ____.
Chapter 6 Review
• The atomic number of an element is the total number of what particles in the nucleus?
• How many electrons does the ion Ca
2+
contain?
• How many electrons are there in the highest occupied energy level of atoms in Group 5A elements?
Chapter 6 Review
• How many electrons are in a rubidium ion, Rb
1+
?
• How many electrons are present in the d sublevel of a neutral atom of nickel?
• What is the usual charge on an ion from Group 7A?