Chemistry 21 June 2016

Chemistry 21 June 2016 Questions Answer keys

The University Of The State Of New York
Regents High School Examination
Physical Setting
Chemistry
Tuesday, June 21, 2016 — 9:15 a.m. to 12:15 p.m., only

1. Which statement describes the charge of an electron and the charge of a proton?

  • (1) An electron and a proton both have a charge of +1.
  • (2) An electron and a proton both have a charge of -1.
  • (3) An electron has a charge of 1, and a proton has a charge of -1.
  • (4) An electron has a charge of 1, and a proton has a charge of +1.
Answer: (4) An electron has a charge of 1, and a proton has a charge of +1. 

2. Which subatomic particles are found in the nucleus of an atom of beryllium?

  • (1) electrons and protons
  • (2) electrons and positrons
  • (3) neutrons and protons
  • (4) neutrons and electrons
Answer: (3) neutrons and protons 

3. The elements in Period 4 on the Periodic Table are arranged in order of increasing

  • (1) atomic radius
  • (2) atomic number
  • (3) number of valence electrons
  • (4) number of occupied shells of electrons
Answer: (2) atomic number 

4. Which phrase describes two forms of solid carbon, diamond and graphite, at STP?

  • (1) the same crystal structure and the same properties
  • (2) the same crystal structure and different properties
  • (3) different crystal structures and the same properties
  • (4) different crystal structures and different properties
Answer: (4) different crystal structures and different properties 

5. Which element has six valence electrons in each of its atoms in the ground state?

  • (1) Se
  • (2) As
  • (3) Kr
  • (4) Ga
Answer: (1) Se  

6. What is the chemical name for H2SO3(aq)?

  • (1) sulfuric acid
  • (2) sulfurous acid
  • (3) hydrosulfuric acid
  • (4) hydrosulfurous acid
Answer: (2) sulfurous acid  

7. Which substance is most soluble in water?

  • (1) (NH4)3PO4 
  • (2) Cu(OH)2
  • (3) Ag2SO4
  • (4) CaCO3
Answer: (1) (NH4)3PO4   

8. Which type of bonding is present in a sample of an element that is malleable?

  • (1) ionic
  • (2) metallic
  • (3) nonpolar covalent
  • (4) polar covalent
Answer: (2) metallic 

9. Which atom has the greatest attraction for the electrons in a chemical bond?

  • (1) hydrogen
  • (2) oxygen
  • (3) silicon
  • (4) sulfur
Answer: (2) oxygen 

10. Which type of reaction involves the transfer of electrons?

  • (1) alpha decay
  • (2) double replacement
  • (3) neutralization
  • (4) oxidation-reduction
Answer: (4) oxidation-reduction 

11. A 10.0-gram sample of nitrogen is at STP. Which property will increase when the sample is cooled to 72 K at standard pressure?

  • (1) mass
  • (2) volume
  • (3) density
  • (4) temperature
Answer: (3) density 

12. Which element is a gas at STP?

  • (1) sulfur
  • (2) xenon
  • (3) potassium
  • (4) phosphorus
Answer: (2) xenon 

13. A 5.0-gram sample of Fe(s) is to be placed in 100. milliliters of HCl(aq). Which changes will result in the fastest rate of reaction?

  • (1) increasing the surface area of Fe(s) and increasing the concentration of HCl(aq)
  • (2) increasing the surface area of Fe(s) and decreasing the concentration of HCl(aq)
  • (3) decreasing the surface area of Fe(s) and increasing the concentration of HCl(aq)
  • (4) decreasing the surface area of Fe(s) and decreasing the concentration of HCl(aq)
Answer: (1) increasing the surface area of Fe(s) and increasing the concentration of HCl(aq) 

14. Which process is commonly used to separate a mixture of ethanol and water?

  • (1) distillation
  • (2) ionization
  • (3) filtration
  • (4) titration
Answer: (1) distillation 

15. A sample of hydrogen gas will behave most like an ideal gas under the conditions of

  • (1) low pressure and low temperature
  • (2) low pressure and high temperature
  • (3) high pressure and low temperature
  • (4) high pressure and high temperature
Answer: (2) low pressure and high temperature 

16. The collision theory states that a reaction is most likely to occur when the reactant particles collide with the proper

  • (1) formula masses
  • (2) molecular masses
  • (3) density and volume
  • (4) energy and orientation
Answer: (4) energy and orientation

17. At STP, which sample contains the same number of molecules as 3.0 liters of H2(g)?

  • (1) 1.5 L of NH3(g)
  • (2) 2.0 L of CO2(g)
  • (3) 3.0 L of CH4(g)
  • (4) 6.0 L of N2(g)
Answer: (3) 3.0 L of CH4(g) 

18. The addition of a catalyst to a chemical reaction provides an alternate pathway that

  • (1) increases the potential energy of reactants
  • (2) decreases the potential energy of reactants
  • (3) increases the activation energy
  • (4) decreases the activation energy
Answer: (4) decreases the activation energy 

19. A sample of water is boiling as heat is added at a constant rate. Which statement describes the potential energy and the average kinetic energy of the water molecules in this sample?

  • (1) The potential energy decreases and the average kinetic energy remains the same.
  • (2) The potential energy decreases and the average kinetic energy increases.
  • (3) The potential energy increases and the average kinetic energy remains the same.
  • (4) The potential energy increases and the average kinetic energy increases.
Answer: (3) The potential energy increases and the average kinetic energy remains the same. 

20. Entropy is a measure of the

  • (1) acidity of a sample
  • (2) disorder of a system
  • (3) concentration of a solution
  • (4) chemical activity of an element
Answer: (2) disorder of a system

21. Which element has atoms that can bond with each other to form ring, chain, and network structures?

  • (1) aluminum
  • (2) calcium
  • (3) carbon
  • (4) argon
Answer: (3) carbon

22. What is the number of electrons shared in the multiple carbon-carbon bond in one molecule of 1-pentyne?

  • (1) 6
  • (2) 2
  • (3) 3
  • (4) 8
Answer: (1) 6 

23. Butanal, butanone, and diethyl ether have different properties because the molecules of each compound differ in their

  • (1) numbers of carbon atoms
  • (2) numbers of oxygen atoms
  • (3) types of functional groups
  • (4) types of radioactive isotopes
Answer: (3) types of functional groups 

24. What occurs when a magnesium atom becomes a magnesium ion?

  • (1) Electrons are gained and the oxidation number increases.
  • (2) Electrons are gained and the oxidation number decreases.
  • (3) Electrons are lost and the oxidation number increases.
  • (4) Electrons are lost and the oxidation number decreases.
Answer: (3) Electrons are lost and the oxidation number increases.

25. Energy is required to produce a chemical change during

  • (1) chromatography
  • (2) electrolysis
  • (3) boiling
  • (4) melting
Answer: (2) electrolysis

26. The reaction of an Arrhenius acid with an Arrhenius base produces water and

  • (1) a salt
  • (2) an ester
  • (3) an aldehyde
  • (4) a halocarbon
Answer: (1) a salt 

27. One acid-base theory defines an acid as an

  • (1) H acceptor
  • (2) H donor
  • (3) H+ acceptor
  • (4) H+ donor
Answer: (4) H+ donor 

28. Which phrase describes the decay modes and the half-lives of K-37 and K-42?

  • (1) the same decay mode but different half-lives
  • (2) the same decay mode and the same half-life
  • (3) different decay modes and different half-lives
  • (4) different decay modes but the same half-life
Answer: (3) different decay modes and different half-lives 

29. Which particle has a mass that is approximately equal to the mass of a proton?

  • (1) an alpha particle
  • (2) a beta particle
  • (3) a neutron
  • (4) a positron
Answer: (3) a neutron

30. Which change occurs during a nuclear fission reaction?

  • (1) Covalent bonds are converted to ionic bonds.
  • (2) Isotopes are converted to isomers.
  • (3) Temperature is converted to mass.
  • (4) Matter is converted to energy.
Answer: (4) Matter is converted to energy.

Download Chemistry 21 June 2016 Questions Answers Keys

Chemistry Examination QuestionLiving Environment January 2014
Living Environment January 2014Scoring Key and Rating Guide

See also: 

0 comments… add one

Leave a Comment