Directed Reading. Section: Combinations of Atoms
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1 Skills Worksheet Directed Reading Section: Combinations of Atoms 1. What is true of the elements found in Earth s crust? a. They usually occur in pure form. b. They generally occur in combination with other elements. c. They usually do not occur in combination with other elements. d. They generally occur in pure form but in combination with other elements. 2. What is a compound? a. a substance made of two or more elements joined by chemical bonds between the atoms of those elements b. a substance made of a single element joined by chemical bonds between the atoms of that element c. a substance made of thousands of elements joined by chemical bonds between the atoms of those elements d. a substance made of two or more subatomic particles joined by physical bonds 3. The properties of a compound are a. the same as those of the elements that make up the compound. b. physically similar to the elements of the compound. c. chemically similar to the elements of the compound. d. different from those of the elements that make up the compound. 4. The smallest unit of a compound that can exist by itself and retain all the compound s chemical properties is a(n) a. mixture. b. atom. c. molecule. d. element. 5. In a molecule of two or more atoms, how are the atoms connected? a. The atoms are chemically bonded together. b. Magnetism connects the atoms. c. The atoms are physically mixed. d. Electrostatic energy bonds the atoms together. Holt McDougal Earth Science 17 Earth Chemistry
2 6. Molecules that are made up of only two atoms are called a. subatomic particles. c. isotopes. b. diatomic molecules. d. chemical formulas. 7. What does O 2 mean? a. It means a diatomic molecule with 2 parts. b. It means an oxygen compound with 2 parts. c. It means a mixture of 2 parts oxygen. d. O is the symbol for oxygen; the subscript 2 indicates the number of oxygen atoms that are bonded together. CHEMICAL FORMULAS 8. In any compound, the elements that make up the compound a. occur in different relative proportions. b. occur in the same relative proportions. c. do not occur in measurable proportions. d. do not occur in the same relative proportions. 9. What is a chemical formula? a. a combination of letters and numbers that shows which elements make up a compound b. the numbers used to show how many chemical and physical bonds a molecule has c. a combination of subscripts and letters that show which electrons make up a mixture d. the letters used to show how many chemical and physical bonds a molecule has 10. What does the chemical formula H 2 O mean? a. Each water molecule has one atom of hydrogen and one atom of oxygen. b. Each water molecule has one atom of hydrogen and two atoms of oxygen. c. Each water molecule has two atoms of hydrogen and two atoms of oxygen. d. Each water molecule has two atoms of hydrogen and one atom of oxygen. 11. In a chemical formula, what does a subscript that follows the symbol for an element indicate? a. half the number of atoms of that element in the molecule b. the number of atoms of that element in the molecule c. double the number of atoms of that element in the molecule d. the number of molecules of that element in an atom Holt McDougal Earth Science 18 Earth Chemistry
3 CHEMICAL EQUATIONS 12. How do elements and compounds form new compounds? a. by being heated and melting together b. by combining through physical reactions c. by combining through chemical reactions d. by dividing through chemical reactions 13. What is a chemical equation? a. an equation that describes the physical reaction of elements and compounds combining to form new compounds b. an equation that describes the chemical reaction of elements that do not combine to form new compounds c. an equation that describes the chemical reaction of elements and compounds combining to form new compounds d. an equation that describes the physical reaction of compounds that do not combine to form new compounds 14. In a chemical equation, what is shown on the left-hand side of the arrow? a. the reactions c. the molecules b. the products d. the reactants 15. In a chemical equation, what is shown on the right-hand side of the arrow? a. the reactions c. the molecules b. the products d. the reactants 16. What does the arrow in a chemical reaction mean? a. gives or yields b. gives and takes c. takes or yields d. takes or makes 17. Explain the equation CH 4 + 2O 2 CO 2 + 2H 2 O. 18. When is a chemical equation balanced? Holt McDougal Earth Science 19 Earth Chemistry
4 19. Why can you not change chemical formulas to balance an equation? 20. What are coefficients? 21. In the equation CH 4 + 2O 2 CO 2 + 2H 2 O, what is the coefficient in 2H 2 O? How is the coefficient used? 22. In the equation CH 4 + 2O 2 CO 2 + 2H 2 O, how is the coefficient in 2O 2 used? CHEMICAL BONDS 23. What are chemical bonds? a. the forces that hold the molecules in atoms together b. the forces that hold the subatomic particles in molecules together with other molecules c. the forces that hold the subatomic particles in atoms in molecules together d. the forces that hold together the atoms in molecules 24. Chemical bonds form because of a. the transmutation of energy. b. the attraction between positive and negative charges. c. the change of matter into energy. d. positive and negative charges repelling each other. Holt McDougal Earth Science 20 Earth Chemistry
5 25. How do atoms form chemical bonds? a. by combining protons b. by either transferring or sharing neutrons c. by either transferring or sharing valence electrons d. by either combining or rearranging valence electrons 26. What is the result of variations in the forces that hold molecules together? a. a wide range of physical and chemical properties b. a wide range of behavioral difficulties c. a narrow range of physical and chemical properties d. virtually nothing 27. When scientists study the interactions of atoms, what can they predict? a. how long it takes for chemical bonds to form b. how subatomic particles will split apart to form other atoms c. which kinds of atoms will form chemical bonds together d. the weather 28. How many valence electrons can a hydrogen atom have? a. 1 b. 2 c. 3 d How can hydrogen reach a more chemically unreactive state? a. by splitting b. by fusing c. by giving up or accepting another proton d. by giving up or accepting another electron 30. What happens when an electron is transferred from one atom to another? a. Only the atom that accepts the electron becomes charged; the other becomes neutral. b. Only the atom that gave up the electron becomes charged; the other becomes neutral. c. Both atoms lose their charge. d. Both atoms become charged. 31. What is an ion? a. an atom or molecule that has a neutral charge b. an atom or molecule that carries a negative or positive charge c. an atom that has at least one extra neutron d. an atom that has at least one extra proton Holt McDougal Earth Science 21 Earth Chemistry
6 32. How many electrons do neutral sodium atoms have? a. 1 b. 11 c. 8 d How many valence electrons does a sodium atom have? a. 8 b. 11 c. 1 d If a neutral sodium atom loses its outermost electron, how many electrons are now in its outermost electron cloud? a. 8 b. 2 c. 11 d When an atom gives up an electron and no longer has equal numbers of positive and negative charges, what does it become? a. a molecule b. an isotope c. neutral d. an ion 36. When a sodium atom releases its valence electron, what does it become? a. a proton b. a sodium isotope c. a positive sodium ion d. a negative sodium ion 37. If a neutral chlorine atom accepts an electron, what happens? a. It now has eight valence electrons, and it becomes a chemically unstable, positively charged chloride ion. b. It now has seven valence electrons, and it becomes a chemically unstable, negatively charged chloride ion. c. It now has eight valence electrons, and it becomes a chemically stable, negatively charged chloride ion. d. It now has seven valence electrons, and it becomes a chemically stable, positively charged chloride ion. Holt McDougal Earth Science 22 Earth Chemistry
7 38. What is an ionic bond? a. the force between charged ions that results from neutron transfer between atoms b. the opposing force between uncharged ions c. the attractive force between ions with the same charge d. the attractive force between oppositely charged ions 39. An ionic compound is formed through the transfer of a. electrons. b. protons. c. neutrons. d. energy. 40. When are most ionic compounds formed? a. when electrons are transferred between atoms of metallic elements b. when neutrons are transferred between atoms of metallic and nonmetallic elements c. when electrons are transferred between atoms of metallic and nonmetallic elements d. when electrons are transferred between atoms of nonmetallic elements 41. Sodium chloride is composed of a. negatively charged sodium ions and positively charged chloride ions. b. positively charged sodium ions and negatively charged chloride ions. c. positively charged sodium ions and chloride ions. d. negatively charged sodium ions and chloride ions. 42. What is a covalent bond? 43. If atoms are sharing electrons, what happens to the positive nucleus of each atom? Holt McDougal Earth Science 23 Earth Chemistry
8 44. What force keeps atoms that share electrons joined? 45. What is a covalent compound? 46. How do two atoms of hydrogen combine with one atom of oxygen to form a water molecule? 47. Why would atoms that are covalently bonded not share electrons equally? 48. What is a polar covalent bond? 49. Explain how water is an example of a molecule that forms because of polar covalent bonds. Holt McDougal Earth Science 24 Earth Chemistry
9 50. What is caused by a water molecule s slightly negative charge at its oxygen end and the slightly positive charge at its hydrogen end? MIXTURES 51. What is a mixture? a. a combination of five or more substances that are not chemically combined b. a combination of two or more substances that are chemically combined c. a combination of two or more substances that are not chemically combined d. a combination of 10 or more substances that are chemically combined 52. The substances that make up a mixture a. keep their individual properties. b. lose their individual properties. c. combine chemically. d. lose their individual chemical properties. 53. Unlike a compound, a mixture a. can be separated into its parts by chemical means. b. cannot be separated into its parts by physical means. c. cannot be separated into its parts by chemical means. d. can be separated into its parts by physical means. 54. To separate a mixture of powdered sulfur, S, and iron, Fe, filings, you can a. use chemical means. b. use a magnet to attract the iron. c. add more chemicals. d. pick out the sulfur by hand. 55. What are heterogeneous mixtures? a. three or more substances that are uniformly distributed b. two or more substances that are not uniformly distributed c. three or more substances that cannot be separated by physical means d. two or more substances that can be separated by physical means Holt McDougal Earth Science 25 Earth Chemistry
10 56. What rock is an example of a heterogeneous mixture of minerals? a. limestone b. feldspar c. quartz d. granite 57. What is a homogeneous mixture? 58. What is a homogeneous mixture of two or more substances uniformly dispersed throughout the mixture? 59. What is dissolved in the solution known as sea water? 60. What is happening in sea water on a molecular level, in terms of positive and negative charges? 61. What is an alloy? Holt McDougal Earth Science 26 Earth Chemistry
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