Chemistry 29 January 2014 Questions Answer Keys
The University Of The State Of New York
Regents High School Examination
Wednesday, January 29, 2014 — 1:15 to 4:15 p.m., only
Directions (1–30): For each statement or question, record on your separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question. Some questions may require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry.
1. What is the approximate mass of a proton?
- (1) 1 u
- (2) 0.0005 u
- (3) 1 g
- (4) 0.0005 g
2. An electron in a sodium atom gains enough energy to move from the second shell to the third shell. The sodium atom becomes
- (1) a positive ion
- (2) a negative ion
- (3) an atom in an excited state
- (4) an atom in the ground state
3. Which particle has no charge?
- (1) electron
- (2) neutron
- (3) positron
- (4) proton
4. Which quantity represents the number of protons in an atom?
- (1) atomic number
- (2) oxidation number
- (3) number of neutrons
- (4) number of valence electrons
5. The element sulfur is classified as a
- (1) metal
- (2) metalloid
- (3) nonmetal
- (4) noble gas
6. The elements in Group 2 have similar chemical properties because each atom of these elements has the same
- (1) atomic number
- (2) mass number
- (3) number of electron shells
- (4) number of valence electrons
7. What is formed when two atoms of bromine bond together?
- (1) a monatomic molecule
- (2) a diatomic molecule
- (3) a heterogeneous mixture
- (4) a homogeneous mixture
8. Gold can be flattened into an extremely thin sheet. The malleability of gold is due to the
- (1) radioactive decay mode of the isotope Au-198
- (2) proton-to-neutron ratio in an atom of gold
- (3) nature of the bonds between gold atoms
- (4) reactivity of gold atoms
9. Which term represents the attraction one atom has for the electrons in a bond with another atom?
- (1) electronegativity
- (2) electrical conductivity
- (3) first ionization energy
- (4) mechanical energy
10. Salt water is classified as a
- (1) compound because the proportion of its atoms is fixed
- (2) compound because the proportion of its atoms can vary
- (3) mixture because the proportion of its components is fixed
- (4) mixture because the proportion of its components can vary
11. Which substance can not be broken down by a chemical change?
- (1) ammonia
- (2) arsenic
- (3) ethane
- (4) propanal
12. Some physical properties of two samples of iodine-127 at two different temperatures are shown in the table below.
These two samples are two different
- (1) mixtures
- (2) substances
- (3) phases of matter
- (4) isotopes of iodine
13. Powdered iron is magnetic, but powdered sulfur is not. What occurs when they form a mixture in a beaker at room temperature?
- (1) The iron retains its magnetic properties.
- (2) The iron loses its metallic properties.
- (3) The sulfur gains magnetic properties.
- (4) The sulfur gains metallic properties.
14. Which property is a measure of the average kinetic energy of the particles in a sample of matter?
- (1) mass
- (2) density
- (3) pressure
- (4) temperature
15. According to the kinetic molecular theory, which statement describes the particles of an ideal gas?
- (1) The gas particles are arranged in a regular pattern.
- (2) The force of attraction between the gas particles is strong.
- (3) The gas particles are hard spheres in continuous circular motion.
- (4) The collisions of the gas particles may result in the transfer of energy
16. The concentration of a solution can be expressed in
- (1) milliliters per minute
- (2) parts per million
- (3) grams per kelvin
- (4) joules per gram
17. Two hydrogen atoms form a hydrogen molecule when
- (1) one atom loses a valence electron to the other atom
- (2) one atom shares four electrons with the other atom
- (3) the two atoms collide and both atoms gain energy
- (4) the two atoms collide with sufficient energy to form a bond
18. Which type of formula represents the simplest whole-number ratio of atoms of the elements in a compound?
- (1) molecular formula
- (2) condensed formula
- (3) empirical formula
- (4) structural formula
19. The coefficients in a balanced chemical equation represent
- (1) the mass ratios of the substances in the reaction
- (2) the mole ratios of the substances in the reaction
- (3) the total number of electrons in the reaction
- (4) the total number of elements in the reaction
20. Systems in nature tend to undergo changes toward
- (1) lower energy and higher entropy
- (2) lower energy and lower entropy
- (3) higher energy and higher entropy
- (4) higher energy and lower entropy
21. Which formula represents an organic compound?
- (1) CaH2
- (2) C4H8
- (3) H2O2
- (4) P2O5
22. Which class of organic compounds contains nitrogen?
- (1) aldehyde
- (2) alcohol
- (3) amine
- (4) ether
23. Which term identifies a type of organic reaction?
- (1) deposition
- (2) distillation
- (3) esterification
- (4) sublimation
24. Which compound is classified as a hydrocarbon?
- (1) butanal
- (2) butyne
- (3) 2-butanol
- (4) 2-butanone
25. In an oxidation-reduction reaction, the number of electrons lost is
- (1) equal to the number of electrons gained
- (2) equal to the number of protons gained
- (3) less than the number of electrons gained
- (4) less than the number of protons gained
26. Which substance is an electrolyte?
- (1) C6H12O6(s)
- (2) C2H5OH(ℓ)
- (3) NaOH(s)
- (4) H2(g)
27. Which energy conversion must occur in an operating electrolytic cell?
- (1) electrical energy to chemical energy
- (2) electrical energy to nuclear energy
- (3) chemical energy to electrical energy
- (4) chemical energy to nuclear energy
28. Which compound yields H+ ions as the only positive ions in an aqueous solution?
- (1) KOH
- (2) NaOH
- (3) CH3OH
- (4) CH3COOH
29. Which statement describes the relative masses of two different particles?
- (1) A neutron has less mass than a positron.
- (2) A beta particle has less mass than a neutron.
- (3) An alpha particle has less mass than a positron.
- (4) An alpha particle has less mass than a beta particle.
30. Which term represents a type of nuclear reaction?
- (1) condensation
- (2) vaporization
- (3) single replacement
- (4) natural transmutation
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