FIRST SEMESTER EXAM REVIEW Chapter 1 Introduction to Chemistry 1. What is chemistry? 2. Identify the independent and dependent variables using the graph above. IV: DV: 3. Write a hypothesis for this experiment. 4. Write a conclusive statement regarding this data. Chapter 2 Energy and Matter 1. Identify the units of the metric system a. Length - b. Mass - c. Volume - d. Know the prefixes from largest to smallest: e. Be able to convert within the metric system: (1) 12.5 m to cm (3) 0.035 kg to g (2) 10521 ml to L (4) 45.6 cm to m
2. Significant figures a. Determine the number of significant figures in measurements (1) 101.000 (2) 0.0023 (3) 0.010500 (4) 10200 b. Use significant figures in calculations (1) 102.345 cm + 22.24 cm = (3) 12.5 cm x 114.2 cm = (2) 45.62 cm - 1.2 cm = (4) 458.3 g/12.6 ml = Chapter 3 Matter Properties and Changes 1. Know the four states of matter and be able to describe each States of Matter Description 2. Compare physical and chemical properties of matter and give an example of each Place a check in the appropriate column below. Property Physical Chemical Color Rusts Length Oxidized Dissolves 3. Compare physical and chemical changes of matter and give an example of each Place a check in the appropriate column: Change Physical Chemical Salt dissolves in water HCl reacts with Mg Piece of copper is cut in half Sugar cube is burned Iron rusts Water evaporates 4. Compare intensive and extensive physical properties Classify each of the following as an intensive property [I] or an extensive property [E]. Mass Density Color Volume 5. Explain the difference between an element, a mixture, and a compound Classify each of the following as an element [E], a compound [C], or a mixture [M]. Gold Water Sugar A chocolate sundae
Seawater hydrogen 6. Explain the difference between homogeneous and heterogeneous mixture. Classify each of the following as either (A) heterogeneous or (B) homogeneous. wood Luck charms freshly brewed coffee salt water and sand sugar water 7. Know the phase changes of matter Melting Freezing Condensation Evaporation Sublimation Deposition Order the substances in the graduated cylinder from lowest to highest density. Identify the following from the graph above: a. Both solid and liquid are present: b. Solid only is present: c. Liquid only present: d. Gas only present: e. Both liquid and gas present: Chapter 4 The Structure of the Atom 1. Define atom
2. List the three subatomic particles, tell where they are located, their relative mass (amu), and the charges of each Subatomic particle Location in atom Charge Mass 3. Define atomic number 4. Define isotope 5. Define mass number 6. Find the missing items in the table below: Name Symbol Atomic number Na Mass number Number protons Number electrons Number of neutrons Nuclear symbol 17 Potassium 20 List the three types of radiation. Write a nuclear equation for the alpha decay of Write a nuclear equation for the beta decay of 149 Sm 62 Describe the current model of the atom. Where are protons, neutrons and electrons located? Identify each of the following as a compound, mixture of compounds and atoms, a mixture of atoms, a mixture of compounds or a mixture of elements.
Chapter 5 Electrons in Atoms 1. Describe what each quantum number indicates about the position of the electron in the atom. 2. Write the electron configuration for an atom of selenium. Use both the regular and noble gas configuration. Regular: Noble Gas: 3. Draw the electron dot structure for an atom of sodium, sulfur and argon. 4. EM Wave A has a wavelength of 200 nanometers (nm). EM Wave B has a wavelength of 500 nanometers (nm). Which wave has a higher frequency? Energy: Chapter 6 The Periodic Table and Periodic Law 1. The horizontal rows are called, the vertical columns are called 2. Know the names of the groups a. (a) Group 1 (c) Group 17 (7A) b. (b) Group 2 (d) Group 18 (8A) 3. Locate the s, p, d, and f blocks Block Groups Block Groups s d p f 4. Locate the transition metals: Groups 5. Be able to differentiate between metals, nonmetals, and metalloids (semi-metals) on the periodic table. Give an example of each. a. Metal: b. Nonmetal: c. Metalloid: 6. What does the term malleable mean? 7. Define electronegativity. 8. Identify the periodic trends for atomic radius and ionization energy. a. Atomic radius as you move across a row on the periodic table. b. Atomic radius as you move down a group on the periodic table. 9. Draw the shape of s and p orbitals. 10. Elements with similar properties are organized into on the periodic table.
Chapter 7 & 8 Ionic Compounds & Covalent Bonding 1. An ionic bond is. 2. A cation is a and an anion is a. 3. A monatomic ion is a and a polyatomic ion is a. 4. Know the charges of the ions in groups 1,2,13,15,16, and 17. 5. Which group of elements is stable and does not form ions? 6. Negative ions form when atoms (gain/lose) electrons. 7. Positive ions form when atoms (gain/lose) electrons. 8. A covalent bond is. 9. Which type of covalent bond is the strongest: single, double or triple? 10. Identify the number of protons, neutrons and electrons in a calcium ion (Ca 2+ ) (a) Protons: (b) Neutrons: (c) Electrons: 11. Draw Lewis structures for molecules and polyatomic ions. (a) H2S (c) SiO2 (b) NCl3 (d) CO2 12. Name a compound when given its formula. (a) HNO3 (e) IF5 (b) XeO3 (f) KMnO4 (c) FeCl3 (g) NO2 (d) HI (h) H2SO4 8. Write the formula of a compound when given its name. 1. potassium chloride 5. calcium hydroxide 2. cobalt (II) oxide 6. sulfur hexafluoride 3. phosphorous trichloride 7. disulfur decafluoride 4. phosphoric acid 8. hydrobromic acid