Earth Science January 2002 Questions Answers Keys.
The University of the State of New York
REGENTS HIGH SCHOOL EXAMINATION
Tuesday, January 22, 2002 — 9:15 a.m. to 12:15 p.m., only
Directions : For each statement or question, select the word or expression that, of those given, best completes the statement or answers the question. Record your answer on the separate answer sheet in accordance with the directions on the front page of this booklet.
1. Which sample of water has the lowest vapor pressure?
- (1) 100 mL at 50°C
- (2) 200 mL at 30°C
- (3) 300 mL at 40°C
- (4) 400 mL at 20°C
2. Which type of matter is composed of two or more different elements that are chemically combined in a definite ratio?
- (1) a solution
- (2) a compound
- (3) a homogeneous mixture
- (4) a heterogeneous mixture
3. A sealed flask containing 1.0 mole of H2(g) and a sealed flask containing 2.0 moles of He(g) are at the same temperature. The two gases must have equal
- (1) masses
- (2) volumes
- (3) average kinetic energies
- (4) numbers of molecules
4. Two basic properties of the gas phase are
- (1) a definite shape and a definite volume
- (2) a definite shape but no definite volume
- (3) no definite shape but a definite volume
- (4) no definite shape and no definite volume
5. The temperature at which the solid and liquid phases of matter exist in equilibrium is called its
- (1) melting point
- (2) boiling point
- (3) heat of fusion
- (4) heat of vaporization
6. Which element has an atom with the electron configuration 2–8–8–2?
- (1) Mg
- (2) Ni
- (3) Ca
- (4) Ge
7. Which type of radiation has neither mass nor charge?
- (1) gamma
- (2) neutron
- (3) alpha
- (4) beta
8. Which list of particles is in order of increasing mass?
- (1) proton → electron → alpha particle
- (2) proton → alpha particle → electron
- (3) electron → proton → alpha particle
- (4) alpha particle → electron → proton
9. Compared to a sodium atom in the ground state, a sodium atom in the excited state must have
- (1) a greater number of electrons
- (2) a smaller number of electrons
- (3) an electron with greater energy
- (4) an electron with less energy
10. Which particles are isotopes of each other?
11. Which electron-dot symbol correctly represents an atom of its given element?
12. The half-life of a radioactive substance is 2.5 minutes. What fraction of the original radioactive substance remains after 10 minutes?
13. Given the unbalanced equation:
Mg(ClO3)2(s) → MgCl2(s) + O2(g)
What is the coefficient of O2 when the equation is balanced correctly using the smallest wholenumber coefficients?
- (1) 1
- (2) 2
- (3) 3
- (4) 4
14. The burning of magnesium involves a conversion of
- (1) chemical energy to mechanical energy
- (2) chemical energy to heat energy
- (3) heat energy to chemical energy
- (4) heat energy to mechanical energy
15. The chemical formula for nickel (II) bromide is
- (1) Ni2Br
- (2) NiBr2
- (3) N2Br
- (4) NBr2
16. Which statement explains why H2O has a higher boiling point than N2?
- (1) H2O has greater molar mass than N2.
- (2) H2O has less molar mass than N2.
- (3) H2O has stronger intermolecular forces than N2.
- (4) H2O has weaker intermolecular forces than N2.
17. The ability of carbon to attract electrons is
- (1) greater than that of nitrogen, but less than that of oxygen
- (2) less than that of nitrogen, but greater than that of oxygen
- (3) greater than that of nitrogen and oxygen
- (4) less than that of nitrogen and oxygen
18. In aqueous solution, a chloride ion is attracted to which end of the water molecule?
- (1) the hydrogen end, which is the positive pole
- (2) the hydrogen end, which is the negative pole
- (3) the oxygen end, which is the positive pole
- (4) the oxygen end, which is the negative pole
19. Which statement best describes the substance that results when electrons are transferred from a metal to a nonmetal?
- (1) It contains ionic bonds and has a low melting point.
- (2) It contains ionic bonds and has a high melting point.
- (3) It contains covalent bonds and has a low melting point.
- (4) It contains covalent bonds and has a high melting point.
21. Which statement is true about the properties of the elements in any one period of the Periodic Table?
- (1) They are determined by the number of neutrons.
- (2) They are determined by the number of electrons in the first shell.
- (3) They change in a generally systematic manner.
- (4) They change in a random, unpredictable manner.
22. Arsenic and silicon are similar in that they both
- (1) have the same ionization energy
- (2) have the same covalent radius
- (3) are transition metals
- (4) are metalloids
23. Which statement explains why the radius of a lithium atom is larger than the radius of a lithium ion?
- (1) Metals lose electrons when forming an ion.
- (2) Metals gain electrons when forming an ion.
- (3) Nonmetals lose electrons when forming an ion.
- (4) Nonmetals gain electrons when forming an ion
24. The atoms of the elements in Group 2 have the same
- (1) mass number
- (2) atomic number
- (3) number of protons
- (4) number of valence electrons
25. Which element has the highest electrical conductivity?
- (1) Mg
- (2) H
- (3) He
- (4) Cl
26. Most metals have the properties of
- (1) brittleness and high ionization energy
- (2) brittleness and low ionization energy
- (3) ductility and high ionization energy
- (4) ductility and low ionization energy
27. Given the reaction:
C6H12O6(s) + 6 O2(g) → 6CO2(g) + 6H2().
How many moles of C6H12O6(s) are needed to produce 24 moles of carbon dioxide?
- (1) 1.0 mole
- (2) 12 moles
- (3) 24 moles
- (4) 4.0 moles
28. Which formula is an empirical formula?
- (1) C2H6
- (2) C4H10
- (3) H2O
- (4) H2O2
29. What is the percent by mass of oxygen in
Ca(OH)2? [formula mass = 74.1]
- (1) 21.6%
- (2) 43.2%
- (3) 45.9%
- (4) 54.1%
30. A closed container holds 3.0 moles of CO2 gas at STP. What is the total number of moles of Ne(g) that can be placed in a container of the same size at STP?
- (1) 1.0 mole
- (2) 1.5 moles
- (3) 3.0 moles
- (4) 0.0 moles
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