3. Which of the following has the longest wavelength? a) X rays b) microwaves c) green light d) UV light
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1 Name Sample Exam 1 Chemistry 118 Part I- Multiple Choice. Please choose the single correct answer. 1. Which of the following statements is false? a) Atoms of the same element can have different numbers of neutrons. b) Atoms of the same element can have different numbers of protons. c) Atoms of the same element can have different mass numbers. d) Atoms of two different elements can have the same number of neutrons. 2. Which of the following is not part of Dalton s atomic theory? a) All matter is composed of indivisible atoms. b) Atoms of different elements differ in size and properties. c) Isotopes of the same element have different chemical properties. d) A chemical reaction occurs when atoms recombine in whole number ratios. 3. Which of the following has the longest wavelength? a) X rays b) microwaves c) green light d) UV light 4. A Lewis dot structure for this atom has five electrons around the symbol. Which of the following could be the atom? a) phosphorus b) xenon c) aluminum d) boron 5. These two elements follow a duet rather than an octet rule. What are they? a) helium and neon b) hydrogen and helium c) sodium and chloride d) this is a trick question: all elements follow an octet rule. 6. Which of the following descriptions is true of ionic compounds? a) individual molecules are formed b) the non-directional nature of the attractive forces results in an extended crystal structure c) their properties are similar to the compounds that compose them d) they are generally formed when nonmetals react with other nonmetals 7. How many moles are in 237 g (about a cup) of H 2 O? a) 13.2 moles b) 4270 moles c) moles d) 6.02 x moles 8. Which of the following is most likely to lose electrons in an ionic compound? a) oxygen (O) b) hydrogen (H) c) lead (Pb) d) carbon (C)
2 9. An experiment was performed to find the number of moles of hydrochloric acid in a sample with the following results: Trial Moles The actual number of moles was later determined to be The above results are: a) both accurate and precise b) accurate but imprecise c) precise but inaccurate d) both inaccurate and imprecise 10. Aspirin has the formula C 9 H 8 O 4. A compound is isolated from sea urchins that also has the formula C 9 H 8 O 4. What can you conclude? a) Sea urchins produce aspirin. b) Sea urchins might produce aspirin, but this isn t sufficient evidence that they do. c) Because aspirin is a fairly small molecule, it is probably present in all living organisms. d) Even if this sea urchin compound is not aspirin, it is likely to be good for headaches since it has the same chemical formula as aspirin. 11. Which of the following statements best describes what happens when chocolate melts? a) This is a physical change, and the molecules move farther apart. b) This is a chemical change, and the molecules move farther apart. c) This is a physical change, and the molecules move closer together. d) This is a chemical change, and the molecules move closer together. 12. Which of the following would be balanced coefficients for the following equation: a) 1, 1, 1 b) 4, 3, 2 c) 12, 10, 6 d) 16, 12, 8 X Al + Y O 2 Z Al 2 O Which of the following pairs of compounds illustrates the law of multiple proportions? a) SO, SO 2 b) CO, CaCO 3 c) H 2 SO 4, H 2 S d) H 2 O, C 12 H 22 O Substance A absorbs blue light, and substance B absorbs yellow light. Which of the following is true? a) The energy gap between the ground and excited states is greater for A than B. b) The energy gap between the ground and excited states is smaller for A than B. c) A must have more electrons than B. d) A must be a noble gas. 2
3 15. What is the molar mass of acetaminophen, shown here? a) 151 g/mol b) 48 g/mol c) 120 g/mol d) 132 g/mol O N H acetaminophen OH Part II- Short Answer 1. Circle all the chemical changes below. Food is metabolized to release energy. A red substance is decomposed by heat to mercury and oxygen. Sodium dropped in water forms sodium hydroxide and hydrogen gas. Water boils on the stove. A hydrogen balloon ignites in the presence of oxygen to form water. Salt dissolves in water. 2. Fill in the missing information (as indicated by? ) in the following table. Atom He-4 An isotope of He-4 with 2 more neutrons? # protons??? #neutrons??? #electrons?? 16 mass number?? Use the models below for this question. (p= protons; n = neutrons; e = electrons) 4 p, 4 n 5 p, 6 n 4 p, 6 n 4 e 5 e 4 e Atom 1 Atom 2 Atom 3 a) What is the relationship between Atom 1 and Atom 3? (One word is sufficient.) b) Write each of the atoms above in the shorthand notation that describes the most common isotope of hydrogen as H-1. Atom 1: Atom 2: Atom 3: 3
4 c) Briefly comment on the proportions of these atoms as they are depicted here. d) How many valence electrons does Atom 2 have? 4. Circle any of the following formulas that could be real compounds. Mg 2 O CsCl BeN CaF 2 CH 5 5. For each of the following compounds, a) Circle the correct type of bonding. b) Predict whether the compound dissolves significantly in water. (Electronegativity values are as follows: C = 2.5; H = 2.1; N = 3.0; Cl = 3.0; Mg = 1.2) a) Type of bonding? b) Dissolves in water? NH 3 ionic polar covalent nonpolar covalent Yes No C 2 H 6 ionic polar covalent nonpolar covalent Yes No MgCl 2 ionic polar covalent nonpolar covalent Yes No 6. Draw the Lewis dot structures for each of the compounds in the previous question in the boxes provided. a) NH 3 b) C 2 H 6 c) MgCl 2 7. Classify each of the following as an element, compound, or mixture (circle). Blood element compound mixture Salt element compound mixture Gold element compound mixture Glass element compound mixture 4
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(1) e.g. H hydrogen that has lost 1 electron c. anion - negatively charged atoms that gain electrons 16-2. (1) e.g. HCO 3 bicarbonate anion
GS106 Chemical Bonds and Chemistry of Water c:wou:gs106:sp2002:chem.wpd I. Introduction A. Hierarchy of chemical substances 1. atoms of elements - smallest particles of matter with unique physical and
EXPERIMENT 12: Empirical Formula of a Compound
EXPERIMENT 12: Empirical Formula of a Compound INTRODUCTION Chemical formulas indicate the composition of compounds. A formula that gives only the simplest ratio of the relative number of atoms in a compound
1. How many hydrogen atoms are in 1.00 g of hydrogen?
MOLES AND CALCULATIONS USING THE MOLE CONCEPT INTRODUCTORY TERMS A. What is an amu? 1.66 x 10-24 g B. We need a conversion to the macroscopic world. 1. How many hydrogen atoms are in 1.00 g of hydrogen?
neutrons are present?
AP Chem Summer Assignment Worksheet #1 Atomic Structure 1. a) For the ion 39 K +, state how many electrons, how many protons, and how many 19 neutrons are present? b) Which of these particles has the smallest
Lewis Dot Structures of Atoms and Ions
Why? The chemical properties of an element are based on the number of electrons in the outer shell of its atoms. We use Lewis dot structures to map these valence electrons in order to identify stable electron
Atomic mass is the mass of an atom in atomic mass units (amu)
Micro World atoms & molecules Laboratory scale measurements Atomic mass is the mass of an atom in atomic mass units (amu) By definition: 1 atom 12 C weighs 12 amu On this scale 1 H = 1.008 amu 16 O = 16.00
19.2 Chemical Formulas
In the previous section, you learned how and why atoms form chemical bonds with one another. You also know that atoms combine in certain ratios with other atoms. These ratios determine the chemical formula