1 INTRODUCTION TO CHEMISTRY 1. the pursuit of chemical knowledge for its own sake 2. the means by which a society provides its members with those things needed and desired 3. the science concerned with the composition of matter and the changes that matter undergoes 4. field of chemistry that is concerned with the composition of matter 5. describe an object that can be seen only under magnification 6. the study of essentially all chemicals containing carbon a. chemistry b. organic chemistry c. pure chemistry d. analytical chemistry e. theory f. biochemistry 7. field of study that is concerned with the chemistry of living organisms 8. a logical approach to the solution of scientific problems 9. applies science to the production of biological products or processes 10. information obtained directly by using your senses 11. a method of testing a hypothesis 12. variable that one changes during an experiment 13. a proposed explanation for what is observed 14. a well-tested explanation for a broad set of observations 15. describes many observations but does not explain them g. observation h. hypothesis i. scientific method j. experiment k. scientific law l. technology m. microscopic n. biotechnology o. manipulated variable Chapter 1 Introduction to Chemistry 19
2 MATTER AND CHANGE Each clue describes a vocabulary term. Read the clues and write the letters of each term on the lines provided. 1. Clue: part of a system having uniform composition and properties. 2. Clue: one- or two-letter designation for an element. (2 words) 3. Clue: another name for a homogeneous mixture. 4. Clue: simplest form of matter that has a unique set of properties. 5. Clue: the amount of matter an object contains. 6. Clue: matter that has a definite shape and volume. 7. Clue: a physical blend of two or more components. 8. Clue: matter that takes both the shape and volume of its container. Write the letters found inside the circles on the lines below. Then unscramble them to find the term that describes matter that has a uniform and definite composition. Scrambled letters: Solution: Chapter 2 Matter and Change 43
4 ATOMIC STRUCTURE 1. 2. 3. 4. 5. 6. 7. 8. 1 defined as 1 2 the mass of a carbon-12 atom central core of an atom, which contains most of the atom s mass a vertical column of elements in the periodic table subatomic particles with no charge positively charged subatomic particles the smallest particle of an element that retains its identity in a chemical reaction the number of protons in the nucleus of an element negatively charged subatomic particles a. isotopes b. neutrons c. atom d. electrons e. atomic number f. atomic mass unit g. group h. nucleus 9. 10. atoms with the same number of protons but different numbers of neutrons an arrangement of elements according to similarities in their properties i. periodic table j. protons Chapter 4 Atomic Structure 91
5 ELECTRONS IN ATOMS Choose the term from the following list that best matches each description. quantum photons hertz Pauli exclusion principle wavelength Hund s rule atomic emission spectrum photoelectrons Aufbau principle quantum mechanical model 1. The lowest-energy arrangement of electrons in a subshell is obtained by putting electrons into separate orbitals of the subshell before pairing electrons. 2. packets/quanta of electromagnetic energy 3. the SI unit of frequency 4. An atomic orbital can hold no more than two electrons. 5. the amount of energy required to move an electron from its present energy level to the next higher one 6. the modern description of the location and energy of electrons in an atom 7. This principle states that electrons enter orbitals of lowest energy first. 8. the distance between two adjacent crests of an electromagnetic wave 9. This is produced by passing the light emitted by an element through a prism. 10. These are sometimes produced when light shines on metals. 114 Core Teaching Resources
6 THE PERIODIC TABLE 1. The highest occupied s and p sublevels are partially filled. a. representative elements 2. The highest occupied s sublevel and a nearby d sublevel contain electrons. b. electronegativity 3. metals having only 2 electrons in the highest occupied energy level c. atomic radius 4. one half the distance between the nuclei of two atoms of the same element when the atoms are joined d. metals 5. decreases for cations and anions from left to right across a period e. ionization energy 6. 7. 8. 9. 10. 11. 12. 13. 14. measures the ability of an atom to attract electrons when the atom is in a compound an atom or group of atoms that has a positive or negative charge elements in which the highest occupied s and p sublevels are filled nonmetals of Group 7A The highest occupied s sublevel and a nearby f sublevel contain electrons. energy required to remove an electron from an atom positively charged ion Group 1A elements good conductors of heat and electric current f. cation g. noble gases h. alkali metals i. inner transition metals j. nonmetals k. ionic radius l. ion m. Group 2A n. transition metal 15. negatively charged ion o. halogens 16. poor conductors of heat and electric current p. anion Chapter 6 The Periodic Table 141
7 IONIC AND METALLIC BONDING 1. compounds composed of cations and anions a. chemical formula 2. the attraction of free-floating valence electrons for positively charged metal ions b. valence electrons 3. the lowest whole-number ratio of ions in an ionic compound c. electron dot structure 4. the electrostatic attraction that binds oppositely charged ions together d. octet rule 5. the number of ions of opposite charge that surround the ion in a crystal e. halide ion 6. negatively charged ions f. formula unit 7. shows the kinds and numbers of atoms in the smallest representative unit of a substance g. ionic bonds 8. 9. 10. 11. 12. 13. a diagram that shows valence electrons as dots a negative ion formed when a halogen atom gains an electron In forming compounds, atoms tend to react so as to acquire the stable electron configuration of a noble gas. electrons in the highest occupied energy level of an element s atoms. a mixture of two or more elements, at least one of which is a metal positively charged ions h. coordination number i. metallic bonds j. ionic compounds k. alloy l. anions m. cations 166 Core Teaching Resources
9 CHEMICAL NAMES AND FORMULAS 1. compounds that contain one or more hydrogen atoms and produce hydrogen ions in solution a. anion 2. an ionic compound that produces hydroxide ions when dissolved in water b. law of multiple proportions 3. any atom or group of atoms that has a positive charge c. base 4. compounds composed of metal cations and nonmetal anions d. ionic compounds 5. composed of two elements and can be either ionic or molecular e. binary compound 6. an ion consisting of a single atom with a positive or negative charge f. monatomic ion 7. 8. 9. 10. Whenever two elements form more than one compound, the different masses of one element that combine with the same mass of the other element are in the ratio of small whole numbers. a tightly bound group of atoms that behaves as a unit and carries a charge In samples of any chemical compound, the masses of the elements are always in the same proportions. any atom or group of atoms that has a negative charge g. cation h. polyatomic ion i. acids j. law of definite proportions 226 Core Teaching Resources
10 CHEMICAL QUANTITIES Select the term from the following list that best matches each description. mole Avogadro s number molar mass 22.4 L percent composition empirical formula standard temperature and pressure (0 C, 1 atm) 1. a description of the relative amounts of each element in a compound 2. the lowest whole-number ratio of the atoms of the elements in a compound 3. the volume occupied by one mole of any gas at STP 4. the mass (in grams) of one mole of a compound 5. the SI unit representing 6.02 10 23 representative particles of a substance 6. 6.02 10 23 particles 7. the temperature and pressure at which one mole of gas occupies a volume of 22.4 L Chapter 10 Chemical Quantities 251
11 CHEMICAL REACTIONS Each clue describes a vocabulary term. Read the clues and write the letters of each term on the lines provided. 1. Clue: the complete reaction of a hydrocarbon with oxygen to produce carbon dioxide and water. 2. Clue: a single compound is broken down into two or more products. 3. Clue: the equation indicating only those particles that actually take part in a chemical reaction in an aqueous solution. 4. Clue: a substance that speeds up the rate of a chemical reaction. 5. Clue: the elements or compounds on the left side of a chemical equation. 6. Clue: ions that do not participate in an aqueous chemical reaction. 7. Clue: reaction in which atoms of one element replace the atoms of a second, less reactive, element in a compound. 8. Clue: a chemical equation that is consistent with the law of conservation of mass. 9. Clue: numbers placed in front of chemical symbols or formulas in a chemical reaction. Write the letters found inside the circles on the lines below. Then unscramble them to find the term used to describe an insoluble salt. Scrambled letters: Solution: a Chapter 11 Chemical Reactions 275