Chemistry Spring Final ReviewName ______

Period _____ Date ______

compounds

electron structures

ionic

ions

noble gas

transfer

Atoms bond in certain proportions to form (1)______. They do so to achieve greater stability by acquiring a (2)______configuration of valence electrons. If the two atoms are a metal and a nonmetal, the metal will (3)______electrons to the nonmetal. Because the resulting particles will then have a different numbers of positively-charged protons and negatively charged electrons they will be electrically charged. Such charged particles are called (4)______. Oppositely charged particles combine, forming (5)______bonds, so that the overall charge of the (6)______compound is zero.

covalent

covalent

covalent

first

ionic

ionic

molecule

precipitate

sharing

It is possible to predict the proportions of atoms that will form a stable ionic compound. For instance, knowing the magnesium (in Group 2) tends to form +2 ions and oxygen (in Group 16) tends to form -2 ions, we can conclude they will join in a 1 to 1 ratio, and thus will have the formula MgO. (The positive ion is always listed (7)______in a chemical formula.)

If the particles lack a stable noble gas configuration of valence electrons and they are both nonmetals, neither will give up electrons. Instead they can achieve greater stability by (8)______electrons, forming (9)______bonds. The resulting particle is called a (10)______or covalent compound. Ions are not formed and are not involved.

Due to the nature of the different types of bonds, ionic and covalent compounds have distinctive properties. (11)______compounds conduct electricity when melted or dissolved; (12)______compounds don't. (13)______compounds, like oil, are often not soluble in water (but some, like sugar, are soluble). (14)______compounds are generally highly soluble in water.

When a chemical reaction takes place, the products of the reaction usually have very different properties than the reactants have. If a solid product forms in a solution (often making the solution look cloudy), we call that solid a (15)______.

groups

left

upper

compound

molecular

nonmetals

molecule

ions

transition

cation

anion

-ide

sodium iodide

Roman numeral

polyatomic

nonmetal

-ide

atoms

Completion

The elements in the periodic table are arranged in vertical columns called (16)______. Metals are on the (17)______and lower sides of the periodic table. Nonmetals are on the right and (18)______sides.

Every substance is either an element or a (19)______. A compound is either (20)______or ionic in nature. Molecular compounds are composed of two or more (21)______. The representative particle of a molecular compound is a (22)______. Ionic compounds are composed of oppositely charged (23)______combined in electrically neutral groupings. The charges of the ions of most elements in groups 1, 2, and 13-17 can be determined by the position of these elements in the periodic table. Most (24)______metals have more than one common ionic charge. Binary ionic compounds are named by writing the name of the (25)______followed by the name of the (26)______. Names of binary compounds end in (27)______. For example, NaI is (28)______.

According to the stock method of naming, when a cation has more than one ionic charge, a (29)______is used in the name.

Ternary ionic compounds contain at least one (30)______ion.

Name the following compounds and tell what type of compound they are (binary ionic, ternary ionic, or binary molecular).

31.FeBr3______

32.Na2SO4______

Write the formulas for the following compounds.

33.sodium chlorate______

34.lead(II) phosphate______

35.magnesium carbonate______

36.ammonium chloride______

State the name and charge of the following polyatomic ions.

37.NO3______

38.SO4______

39.NH4______

40.CO3______

41.PO4______

42.MnO4______

43.ClO3______

44.C2H3O2______

45.OH______

  1. What does "kinetic" refer to?
  1. What are the three assumptions of the Kinetic Theory?
  1. Define absolute zero and give its value in Kelvin and Celsius.
  1. Define evaporation, condensation, freezing, melting, sublimation and deposition.
  1. Define temperature in terms of the Kinetic Theory.
  1. Define vapor pressure, gas pressure, melting point, boiling point, and phase change.
  1. Differentiate gases, liquids and solids. Describe them in terms of particle motion and their characteristics.
  1. What is vapor pressure? How does a change in temperature affect vapor pressure?
  1. What happens to water particles when water boils?
  1. What happens to a solid's particles when the substance melts?
  1. How does air pressure affect boiling point?
  1. How does atmospheric pressure vary with altitude?
  1. How will the temperature of a boiling liquid change if more heat is added?
  1. In what different physical states can a substance be found?
  1. What are coefficients? What do they have to do with moles?
  1. What is a mole?
  1. What is molar mass? Where do you find the molar mass of an element?
  1. What are hydrogen bonds? How do the hydrogen bonds of water differ from water's covalent bonds?
  1. What is surface tension, and why does water have high surface tension?
  1. Contrast unsaturated, saturated, and supersaturated solutions.
  1. Contrast dilute and concentrated solutions.
  1. How does temperature affect the solubility of gases in water? How does temperature affect the solubility of solids in water?
  1. What is concentration, as it refers to solutions?
  1. What is molarity and what symbol is used for it?
  1. What are some properties of acids? Of bases?
  1. What is an electrolyte?
  1. What makes an acid strong? What makes a base strong?
  1. Of what are hydrocarbons made?
  1. What process is used to separate the components of curde oil? What property of these compounds allows them to be separated by this method?
  1. What prefixes are used (up to 10) to indicate the number of carbons in a chain?
  1. What suffixes are used to indicate the types of bonds between carbon atoms?
  1. What prefix is used to indicate a cyclic alkane?

Give the correct name for each of the following compounds.

  1. CH3CH2CH2CH2CH2CH3
  1. CH3CH=CHCH2CH3
  1. Why are there so many more organic compounds than inorganic compounds?
  1. How do alkanes, alkenes, and alkynes differ from each other?

Explain what makes each of the names listed below incorrect.

  1. cycloethane
  1. methene
  1. 1-methylpropane
  1. 4-pentene
  1. 4-propyne

Draw the structures of the following compounds:

  1. 2 pentyne
  1. 3-propyl hexane
  1. 1,3-dimethylcyclohexane
  1. 4-ethyl-2,6-dimethyl-2-heptene
  1. Name this compound: ______

CH3 CH3

CH3 – CH – C – CH2 – CH2 – CH3

CH3

Explain how the two terms in each of the following pairs differ from each other.

  1. organic chemistry and biochemistry
  1. monosaccharides and polysaccarides
  1. cellulose and starch
  1. aerobic and anaerobic
  1. Provide the chemical reaction that describes photosynthesis.

______+ ______ ______+ ______

  1. What are two other "things" needed for the photosynthesis reaction to work?
  1. From where does almost all the energy that supports life on earth originate?
  1. What is the process that converts light energy into chemical energy and thus makes it usable by organisms?
  2. Which type of organism can use the sunlight directly as their energy source and can fix carbon?
  1. What types of cells perform photosynthesis – animal, plant, fungus, all, or none?
  1. What types of cells respire (perform respiration) – animal, plant, fungus, all, or none?

103. What are the two types of anaerobic respiration?

104. What is the "purpose" of respiration?

Use each of the terms below just once to complete the following sentences.

alpha particle

beta particle

gamma ray

radioactivity

105)The spontaneous emission of radiation by a nucleus is known as ______.

106)A(n) ______is a high-energy form of electromagnetic radiation commonly released during radioactive decay.

107)A(n) ______is a high-energy electron released from a nucleus during radioactive decay.

108)A(n) ______consists of a helium nucleus.

------

alpha

aluminum foil

beta

concrete

gamma

helium

high energy electrons

lead

mass

negative

protons

radioactive

Isotopes with unstable nuclei are (109)______. The radiation they emit may be alpha, (110)______, or gamma. (111)______radiation consists of alpha particles (positively charged (112)______nuclei) that are easily stopped by a sheet of paper. Because an alpha particle consists of two (113)______and two neutrons, but no electrons, it has a +2 charge. Beta radiation is composed of fast-moving particles, which are (114)______and usually carry a (115)______charge. Beta radiation is more penetrating than alpha radiation; it is stopped by (116)______. (117)______radiation is electromagnetic radiation similar to visible light, but much more energetic. Gamma radiation has no (118)______or charge. It is extremely penetrating. (119)______and (120)______reduce the intensity of gamma radiation but do not completely stop it.

True/False

121)Gamma radiation has a negative charge.

122)When a beta particle is emitted, the atomic number increases by 1, and the mass number stays the same.

123)When a radioactive nucleus emits an alpha particle, its atomic number decreases by 4, and its mass number decreases by 2.

124)When a gamma ray is emitted, the atomic mass and atomic number both increase.

Answer the following questions

125)What is the correct nuclear notation for the isotope oxygen-15?

126)What is the most difficult type of radiation to block out?

127)What does the subscript on the nuclear symbol for the alpha particle, He, mean?

128)After an isotope decays by the loss of a beta particle, it has one more proton. Where did the extra proton come from?

129)What is the nuclear symbol for an alpha () particle?

130)What is the nuclear symbol for a beta () particle?

Complete each of the following nuclear equations.

131) C   + _____

132) Ra   + ______

133) Th   + ______

134) Fr  He + ______

135) Why is nuclear fusion regarded as a better source of energy for future human needs than is nuclear fission?

______

______

______

Fill in the blank.

energy

energy

heat

helium

hydrogen

neutron

neutrons

nuclear accidents

nuclear fission

nuclear fusion

radioactive waste

smaller nuclei

(136)______is the process by which a single large nucleus breaks apart into two smaller nuclei.

Three different products formed in any nuclear fission reaction are (137)______, (138)______, and (139)______. If a neutron begins a nuclear chain reaction, then one product of that reaction must be a(n) (140)______.

Two major concerns people have about nuclear reactions are the possibility of (141)______and the issue of how to dispose of (142)______.

(143)______is the reaction that occurs when two small nuclei join together to form a larger nucleus. The sun's (144)______is produced when (145)______nuclei fuse to make (146)______nuclei.

Although fusion is cleaner, safer, and more efficient than fission for producing energy, it is not currently used to produce energy because of the large amount of (147)______required to start the reaction.