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Transcript
Ch 4 Review
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. The weighted average of the atomic masses of an element’s naturally occurring isotopes is called the
a. average atomic number.
c. average atomic unit.
b. average atomic mass.
d. average mass number.
____
2. What is an atom that has a different number of neutrons than other atoms of the same element?
a. ion
c. isotope
b. electron
d. molecule
____
3. What are counted in an atom to determine mass number?
a. neutrons
c. protons and electrons
b. protons and neutrons
d. electrons
____
4. What is the atomic number of an element?
a. the number of protons and neutrons
b. the number of valence electrons
c. the number of neutrons
d. the number of protons
5. Elements are arranged on the periodic table
a. in order of molecular numbers.
b. in order of atomic numbers.
c. alphabetically.
d. randomly.
____
____
6. What forces hold together the atoms in molecules?
a. chemical mixtures
c. gravity fields
b. magnetic fields
d. chemical bonds
____
7. When elements and compounds combine to form new compounds, the reaction is described in a ____
a. chemical mixture.
c. gravity field.
b. chemical equation.
d. chemical bond.
____
8. How many atoms of sodium (Na) are there in the formula for table salt NaCl?
a. 2
c. 1
b. 3
d. 0
____
9. What does “2” mean in the formula for water H2O?
a. two molecules of water
c. two atoms of hydrogen
b. two molecules of hydrogen
d. two atoms of oxygen
____ 10. How do the electrons in atoms form chemical bonds?
a. They are either shared or transferred between atoms.
b. They are shared but not transferred between atoms.
c. They are neither shared nor transferred between atoms.
d. They are transferred but not shared between atoms.
____ 11. Density, color, and boiling point are examples of
a. chemical descriptors.
c. physical properties.
b. chemical properties.
d. physical science.
____ 12. Where are electrons found in atoms?
a. in the electron sphere
b. in the electron zone
c. in the atomic ring cycle
d. in the electron cloud
____ 13. In the chemical formula CO2, what does the small 2 mean?
a. 2 carbon atoms
c. 2 carbon dioxide molecules
b. 2 carbon dioxide atoms
d. 2 oxygen atoms
____ 14. Two types of chemical bonds are
a. positive and negative.
b. ionic and covalent.
c. atomic and covalent.
d. ionic and coefficient.
____ 15. How do compounds differ from mixtures?
a. Compounds are composed of chemically bonded substances; mixtures are composed of
substances that are not bonded chemically.
b. Mixtures are composed of chemically bonded substances; compounds are composed of
substances that are not bonded chemically.
c. Compounds are composed of physically bonded substances; mixtures are composed of
substances that are not bonded chemically.
d. Mixtures are composed of chemically bonded substances; compounds are composed of
solutions.
____ 16. What describes how substances react to form new substances?
a. chemical properties
c. physical properties
b. physical descriptions
d. chemical bonds
____ 17. How are the elements in the periodic table arranged?
a. in order of atomic charge
c. in order of subatomic particles
b. in order of atomic number
d. in alphabetical order
____ 18. The attractive force between oppositely charged ions that result from the transfer of electrons from one atom
to another is known as
a. a covalent bond.
c. an atomic bond.
b. a physical bond.
d. an ionic bond.
____ 19. Within each column, or group, on the periodic table, the different elements’ atoms usually have the same
number of
a. electrons.
c. atomic numbers.
b. valence electrons.
d. mass numbers.
____ 20. What are used to balance chemical equations?
a. chemical formulas
c. coefficients
b. exponents
d. superscripts
____ 21. Chemical properties of matter are characteristics
a.
b.
c.
d.
of subatomic particles that can be observed.
that can be observed without changing substances.
that describe reactions between substances that produce new substances.
that can only be observed through experimentation.
____ 22. Physical properties of matter are characteristics that
a. can be observed without changing the composition of substances.
b. describe reactions between substances.
c. describe reactions between unreactive substances.
d. can be observed only after changing the composition of substances.
____ 23. What makes an atom an isotope?
a. having a different number of protons than other atoms of the same element
b. having a different number of neutrons than other atoms of the same element
c. having the same number of neutrons as other atoms of the same element
d. having the same number of protons and electrons
____ 24. The two most common elements in Earth’s crust are
a. nitrogen and carbon.
c. silicon and oxygen.
b. carbon and oxygen.
d. nitrogen and oxygen.
____ 25. How many hydrogen atoms are in the chemical formula C6H12O6?
a. 6
c. 12
b. 24
d. 18
____ 26. Atoms form chemical bonds by
a. transferring protons from one atom to another.
b. transferring or sharing valence electrons between atoms.
c. transferring or sharing neutrons from one atom to another.
d. combining reactive chemical properties.
____ 27. Which of the following is NOT an example of a mixture?
a. an alloy of two or more metals
c. sea water
b. carbon dioxide
d. granite
____ 28. What numbers are used to balance chemical equations?
a. exponents
c. subscripts
b. imaginary numbers
d. coefficients
____ 29. An atomic mass unit is the approximate mass of
a. a proton or neutron, equaling 1 amu.
b. an electron or neutron, equaling 1 amu.
c. a proton or neutron, equaling 10 amu.
d. an electron, equaling 1 amu.
Matching
Match each item with the correct statement below.
a. negatively charged subatomic particle
b. characteristics that describe how a substance reacts with other substances to form new
substances
c. characteristics that can be observed without changing the composition of the substance
d. subatomic particle without charge
e. positively charged subatomic particle
____ 30. chemical properties
____ 31. neutron
____ 32. proton
____ 33. physical properties
____ 34. electron
Match each item with the correct statement below.
a. the smallest unit of an element that maintains all of the element’s chemical properties
b. two or more substances that are not combined chemically
c. a substance made of two or more chemically bound elements
d. a solution of two or more metals
e. two or more substances uniformly dispersed in a mixture
____ 35. alloy
____ 36. compound
____ 37. solution
____ 38. mixture
____ 39. molecule
Match each item with the correct statement below.
a. homogeneous mixture of two or more substances uniformly dispersed throughout the
mixture
b. number of protons in the nucleus of an atom
c. atom or molecule that has gained or lost electrons
d. number of protons and neutrons in the nucleus of an atom
e. subatomic particle without charge
f. two or more chemically bonded elements
g. negatively charged subatomic particle
h. smallest unit of matter that retains chemical properties
i. positively charged subatomic particle
j. atom with the same number of protons but a different number of neutrons as other atoms
of the element
____ 40. neutron
____ 41. proton
____ 42. isotope
____ 43. solution
____ 44. molecule
____ 45. compound
____ 46. electron
____ 47. mass number
____ 48. atomic number
____ 49. ion
Match each item with the correct statement below.
a. the number of protons plus the number of neutrons in an atom
b. an atom or molecule that has gained or lost one or more electrons
c. the number of protons in an atom’s nucleus
d. a substance composed of two or more elements joined by chemical bonds
e. the smallest unit of a substance that retains all of its chemical properties
____ 50. compound
____ 51. atomic number
____ 52. molecule
____ 53. ion
____ 54. mass number