Chemistry
Ms. Boon
Name: ___________________________
Period: ________ Date:______________
Chemistry Benchmark 1 Study Guide
Unit 1: The Atom and Periodic Table. The periodic table displays the elements in increasing atomic number and shows patterns in the physical
and chemical properties of the elements and how they relate to atomic structure.
1a. I can relate the position of an element in the periodic table to its atomic number and atomic mass. Practice: pp. 86 #1-4, pp. 89 #5, 6, 8., pp.
154 #1, 6
 Draw a diagram of an atom and label the protons, neutrons, and electrons. Describe the charges of each subatomic particle.
 Define atomic number and atomic mass. What determines an atom’s atomic number? How does this relate to the periodic table?
 Using the periodic table, how do you know how many protons, neutrons, and electrons an atom of a certain element has?
 How are elements arranged on the periodic table? Are they arranged by atomic mass or atomic number or something else?
1b. I can find the metals, semimetals, and nonmetals on the periodic table. (See pp. 120-121, 124-131)
 Label the metals, nonmetals, and semimetals on the periodic table.
 Describe the location of metals, semimetals, and non-metals as a trend statement.
 List the major properties of each. (Examples: shininess, conductivity, state of matter, type of ion formed.)
1c. I can use the periodic table to identify halogens, noble gases, alkali metals, alkaline earth metals and transition metals, trends in ionization
energy, electronegativity, and the relative sizes of ions and atoms.
 Define periods and group on the periodic table. Remember, elements in the same group have similar chemical properties.
 Label the halogens, noble gases, alkali metals, alkaline earth metals, and transition metals.
 List the physical properties of elements in the above groups. (Examples: number of valence electrons, reactivity, state of matter) (pp. 124130, pp. 154 #2, 3, 4, 5, 9)
 Define and explain the trends in atomic radii, ionization energy, and electronegativity. Label the trends on the periodic table using arrows.
Be able to take any three elements and put them in order of increasing or decreasing atomic radii, ionization energy, or electronegativity.
(pp. 132-138, pp. 155 #10-12)
Unit 2: Chemical Bonds. Chemical bonding is caused by different electrostatic force (opposite charges attract) between valence electrons of
different atoms.
1d. I can use the periodic table to determine the number of electrons available for bonding. (p. 154 #8, p. 165 #1-2, 6-7, 10)
 Define Key Vocabulary: (1) valence electron; (2) octet rule; (3) anion; (4) cation; (5) Lewis dot diagram
 Label the periodic table with the # of valence electrons in atoms of each group. Draw a Lewis Dot Diagram of any main group (1, 2, 1318) element. Use the Lewis Dot Diagrams to make ion formulas. (Example: Chlorine has 7 valence electrons so it gains 1 electron to
form the Cl- ion.)
 What type of ions do metals form? What type of ions do non-metals form? Why don’t the noble gases form ions?
2c. I know salt crystals, such as NaCl, are repeating patterns of positive and negative ions held together by electrostatic attraction. (pp. 186 #1, 4,
5, 6, 8-11.)
 Define Key Vocabulary: anion, cation, ionic bond, electrostatic attraction, crystal lattice, octet rule, criss-cross rule
 Remember: ionic bonds involve the transfer of electrons from positive cation (metal) to negative anion (non-metal) – opposites attract!
 Practice using the Criss-Cross rule to make ionic compound formulas with the correct proportion of cations and anions.
2e. I know how to draw Lewis dot structures of molecules. (pp. 217 #30, 32, 40)
 Use the octet rule to draw the Lewis Dot structures of molecules with single, double, or triple bonds.
2b. I know chemical bonds between atoms in molecules such as H2, CH4, NH3, N2, Cl2, and many large biological molecules are covalent. (pp. 220
#3, 7, 9)
 Define Key Vocabulary: (1) macromolecule; (2) covalent compound; (3) diatomic molecule; (4) single covalent bond; (5) double covalent
bond; (6) triple covalent bond.
 Covalent bonds form between nonmetals. We use Lewis Dot Structures of molecules to diagram covalent bonding.
 Living things like animals, plants, fungi, bacteria, and viruses are made of molecules held together by covalent bonds.
2a. I know the properties of covalent and ionic compounds and bonds. (pp. 385-386, 389, pp. 392 #1, 3, 5, 10, 11; pp. 216 # 15, pp. 217 #39)
 Define Key Vocabulary: (1) covalent bond; (2) ionic bond; (3) polar covalent bond; (4) nonpolar covalent bond; (5) electrostatic attraction
(6) chemical compound; (7) molecule
 Compare and Contrast: properties of covalent compounds/bonds with properties of ionic compounds/bonds (Hint: Use your Venn
diagram notes and your Ionic or Covalent Lab.)
Unit 3: Chemical Reactions. The conservation of atoms in chemical reactions leads to the principle of conservation of matter and the ability to
calculate the mass of products and reactants.
3a. I know how to describe chemical reactions by writing balanced equations. pp. 269 #1-4, pp. 271 #1-3, pp. 273 #1-3, pp. 274 #5-10
 What is the law of conservation of mass and how does it relate to balancing chemical equations? Practice balancing equations!
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