Name: Period: Row:
Chemistry Unit 1 Study Guide This study guide is meant to help you prepare for the exam. It is worth an extra credit 5% applied to your exam score and due the day of the exam. Chapter 1 1. What is matter? 2. What is density? 3. What would the density be of 14.2 g of Al which displaced the water 7ml? 4. What are the 6 steps of the scientific method in order? 5. What is the difference between an observation and an inference? 6. When does a hypothesis become a theory? (be specific)
Chapter 2 1. How many liters are there in 45000 ml? 2. How many cm are in 200mm? 3. How do you write 16500 in scientific notation? 4. How would you round 0.98970 to 2 sig figs and scientific notation? 5. Convert 72 g to mg 6. What is the equation for percent error?
Name: Period: Row: 7. How do you calculate percent error if you got a density of 5.6 g/ml and the density should have been 5.1g/ml? Chapter 3/4 1. Draw a picture of an atom and label the protons, neutron, electrons and nucleus and give the charge of each particle
2. Explain the difference between and give an example of a a. Chemical property b. Physical property 3. Explain how energy states vary and how the molecules look in a(an) a. Solid b. Liquid c. Gas 4. What does the equation for conservation of mass(matter) state? 5. What is an element? 6. What is a compound? 7. What does the atomic number tell us? 8. What does the mass number tell us?
Name: Period: Row: 9. What is the number of protons in Nitrogen? Electrons? Neutrons?
Chapter 5 1. What does Bohr’s model tell us? 2. What is a valence electron? 3. How many valence electrons does Chlorine have? 4. What is the electron configuration for a. Zinc (Zn) b. Sulfur (S) c. Tin (Sn) 5. Draw the Lewis dot structure for a. Krypton b. Calcium c. Sodium Chloride d. Carbon Dioxide
Chapter 6 1. As you move down the period (row) from left to right, what happens to atomic radii?
Name: Period: Row: 2. As you move down the period (row) from left to right, what happens to electronegativity? 3. As you move down the period (row) from left to right, what happens to ionization energy? 4. As you move down the group (column) from top to bottom, what happens to atomic radii? 5. As you move down the group (column) from top to bottom, what happens electronegativity? 6. As you move down the group (column) from top to bottom, what happens to ionization energy? 7. Define: a. Atomic radii b. Electronegativity c. Ionization energy 8. Give 3 examples of alkali metals. Which group # are they? 9. Give 3 examples of alkaline earth metals. Which group # are they? 10. Give 3 examples of halogens. Which group # are they? 11. How many valance electrons does each group have? a. Alkali metals b. Alkaline earth metals c. Halogens
Name: Period: Row: d. Noble gases Chapter 8 1. What is an ionic bond? 2. Which groups (names and numbers) bond ionically? (elements?) a. . b. . c. . 3. What is the oxidation number? 4. If you had Magnesium Chloride, how would you write that so the oxidation numbers are balanced? 5. How would you write Ammonium Chloride so that the oxidation numbers were balanced? 6. How are Metallic bonds described as? Why? 7. What is a metal alloy? 8. Give the formula for iron (III)chloride Chapter 9 1. What is a covalent bond? 2. Which groups of elements (names and #) bond covalently? 3. Draw the Lewis dot structure for N2
Name: Period: Row: 4. Why do molecules in organic compounds bond covalently? 5. Give the 3 elements found in nature that bond covalently. 6. How strong are covalent bonds? 7. Explain the difference between an exothermic and endothermic reaction 8. Write the molecular formula for a. Disulfur trioxide b. Dinitrogen monoxide c. Phosphorous Perchlorate 9. Describe what bond would result from a. Metal-nonmetal b. Nonmetal-nonmetal c. Metal-metal 10. What is a polar covalent bond? Give an example 11. What is a nonpolar covalent bond? Give an example
Chapter 10 1. Give 4 examples of chemical change you can observe in a lab 2. Explain the difference between the types of reactions
Name: Period: Row: a. Synthesis b. Decomposition c. Single Replacement d. Double Replacement 3. Write the skeleton equations and balance for a. Lithium + gold(III)chloride lithium chloride + gold b. Iron + tin(IV) nitrate iron(III) nitrate + tin c. Aluminum carbonate aluminum oxide + carbon dioxide d. Silver nitrate + sodium sulfide silver sulfide + sodium nitrate Chapter 12 1. What does it mean to have a ‘mole ‘ of something? 2. What is molar mass ? 3. How many atoms in 2.5 mol of Zn? 4. How many molecules in 11.5 mol of H2O?