1. Chapter 9 - Review States of Matter

2. 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?

3. 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?

4. 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?

5. 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?

6. Chapter 9 - Review
What is the volume occupied by 14.0 x 1023 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?

7. 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 ___.

8. 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 oC, or water at 373 K
Describe the kinetic theory of gases.

9. 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 ____

10. 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.

11. 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 ___.

12. 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?

13. 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?

14. 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?

15. Chapter 9 - Review
The first particles to evaporate from a liquid are ____.
Which of the following will evaporate fastest: water at 20 oC, or water at 40 oC?
If a liquid is sealed in a container and kept at constant temperature, how does it’s vapor pressure change over time?

16. 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 ______.

17. 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 oC instead of 100 oC by ___.

18. 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 _____.

19. 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.

20. 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?

21. Chapter 9 - Review
The direct change of a substance from a solid to a gas is called ____.

22. Chapter 10 – Review The Behavior of Gases

23. 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?

24. 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 _______.

25. 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?

26. 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?

27. 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?

28. Chapter 10 - Review
A gas occupies a volume of 0.7 L at 10.1 kPa. What volume will the gas occupy at 101 kPa?
A sample of gas occupies 40 mL at –123 oC. What volume does the sample occupy at 27 oC?
What type of changes could cause an increase in the pressure of a gaseous system?

29. 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 _____.

30. 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 _____.

31. 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?

32. 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?

33. 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?

34. Chapter 10 - Review
If a balloon containing 1000 L of gas at 50 oC and 101 kPa rises to an altitude where the pressure is 50.5 kPa and the temperature is 10 oC, the volume of the balloon under these new conditions would be _____.

35. 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?

36. 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 PV/T

37. 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?

38. Chapter 10 - Review
At a certain temperature and pressure, 0.20 mol of CO2 has a volume of 3.1 L. A 3.1 L sample of hydrogen at the same temperature and pressure contains ______ molecules.
Under what conditions is the behavior of a real gas like that of an ideal gas?

39. 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?

40. 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?

41. 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 PHe = 84 kPa and PCO2 = 0.1 kPa?

42. Chapter 10 - Review
When a container is filled with 3 moles of H2, 2 moles of O2, and 1 mole of N2, the pressure in the container is 8787 kPa. What is the partial pressure of O2?

43. 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 _____.

44. 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 oC. What is the partial pressure of the nitrogen?
Which gas would effuse most rapidly: chlorine or hydrogen?

45. Chapter 10 - Review
Which of the following atoms would have the greatest velocity if each atom had the same kinetic energy: hydrogen or bromine?

46. 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?

47. Chapter 5 - Review Chemical Names and Formulas

48. 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 Sr2+; Kr; Br1-?

49. 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 ____.

50. 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?

51. 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; BaI2; N2O4
Which represents a molecular compound: Xe; ZnO; SO2

52. 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.

53. Chapter 5 Review What information is obtained about the formula C2H6O?
What is the charge on a formula such as K2O?
Ionic compounds are composed of ____ and ____ ions.
What information does a molecular formula give?

54. Chapter 5 Review
Which of the following pairs of substances best illustrates the Law of Multiple Proportions: NO and NO2; P2O5 and PH3
What is the usual charge on an ion from Group 7A?
What is the charge on an ion of: potassium; strontium; oxygen

55. Chapter 5 Review Give the name for the following ions: Fe2+ and Fe3+
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

56. 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: OH1-; O2-
Polyatomic ions are tightly bound groups of _____.

57. Chapter 5 Review Name: CrO42- and Cr2O72-
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, ZrO2?

58. Chapter 5 Review What is the correct name for the N3- ion?
What is the correct formula for potassium sulfite?
What is the correct formula for barium chlorate?
Ternary ionic compounds contain three different ______.

59. 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 Au3+ and S2-?

60. Chapter 5 Review What is the ionic charge on the thorium ion in ThO2?
What is the formula of the ionic compound from combining Sc3+ and S2-?

61. Chapter 5 Review Name SnF4 and Na2O.
Which of the following contains the lead (IV) ion: Pb4O3; Pb2O; PbO2
Which contains the Mn3+ ion: Mn2O3 or Mn3O2

62. 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 _______.

63. Chapter 6 Review “The Periodic Table”

64. 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.

65. 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 _____.

66. Chapter 6 Review
In which of the following groups of ions are the charges all shown correctly: a) Li1-, O2-, S2+, or b) Ca2+, Al3+, Br1-?
Which of the following elements are nonmetal: Pt, V, Li, and Kr
Know the characteristics of cations and anions.

67. 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?

68. 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?

69. 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?

70. 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?

71. 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?

72. Chapter 6 Review
What element has the electron configuration of 1s22s22p63s23p2?
In which of the following sets are the charges given correctly for all the ions: a) Na1+, Mg1+, Al1+, or b) K1+, Sr2+, O2-?
Which of the following elements has the smallest ionic radius: a) Li, or b) K?

73. 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?

74. 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 ____.

75. 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?

76. 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 ____.

77. 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 ____.

78. 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 Ca2+ contain?
How many electrons are there in the highest occupied energy level of atoms in Group 5A elements?

79. Chapter 6 Review How many electrons are in a rubidium ion, Rb1+?
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?

80. Chapter 6 Review
End of Chapter 6 Review