Regents Review Questions from August 2015...A) protons lost B) neutrons lost C) neutrons gained D)...
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Name: Regents Review Questions from August 2015 A) electron-positive, neutron-negative, proton-neutral B) electron-negative, neutron-neutral, proton-positive C) electron-negative, neutron-positive, proton-neutral D) electron-neutral, neutron-positive, proton-negative 1. Which subatomic particles are paired with their charges? A) Cr B) Cu C) Ni D) Se 2. In the ground state, an atom of which element has two valence electrons? A) absorb energy B) absorb positrons C) emit energy D) emit positrons 3. The atoms in a sample of an element are in excited states. A bright-line spectrum is produced when these atoms A) Positrons are located in shells outside the nucleus. B) Neutrons are located in shells outside the nucleus. C) Protons are located in orbitals outside the nucleus. D) Electrons are located in orbitals outside the nucleus. 4. Which statement describes a concept included in the wave-mechanical model of the atom? A) atomic mass B) molar mass C) number of neutrons per atom D) number of protons per atom 5. All elements on the modern Periodic Table are arranged in order of increasing A) ammonia B) chlorine C) neon D) nitrogen 6. At STP, which substance is a noble gas? A) different molecular structures and different properties B) different molecular structures and the same properties C) the same molecular structure and different properties D) the same molecular structure and the same properties 7. At STP, oxygen exists in two forms, and . These two forms of oxygen have A) decomposition B) distillation C) sublimation D) vaporization 8. Which term identifies a type of chemical reaction? A) Sodium has a melting point of 371 K. B) Sodium has a molar mass of 23 grams. C) Sodium can conduct electricity in the liquid phase. D) Sodium can combine with chlorine to produce a salt. 9. Which statement describes a chemical property of sodium? A) polonium B) sulfur C) selenium D) tellurium 10. Based on Table S, an atom of which element has the weakest attraction for electrons in a chemical bond? A) Energy is absorbed as a bond is formed. B) Energy is absorbed as a bond is broken. C) Energy is released as a bond is formed. D) Energy is released as a bond is broken. 11. Given the balanced equation: Which statement describes what occurs during this reaction? A) O and Se B) O and Sr C) O and H D) O and P 12. Which atoms will bond when valence electrons are transferred from one atom to the other? A) B) C) D) 13. Which sample of matter is a mixture? A) increase the energy content of the gas sample B) produce strong attractive forces between the gas particles C) result in a net loss of energy by the gas sample D) transfer energy between the gas particles 14. According to kinetic molecular theory, collisions between gas particles in a sample of an ideal gas A) ethane B) propanone C) silicon D) water 15. Which substance can not be broken down by a chemical change? A) B) C) D) 16. Which particle has two neutrons?
Transcript of Regents Review Questions from August 2015...A) protons lost B) neutrons lost C) neutrons gained D)...
Name: Regents Review Questions from August 2015
A) electron-positive, neutron-negative, proton-neutralB) electron-negative, neutron-neutral, proton-positiveC) electron-negative, neutron-positive, proton-neutralD) electron-neutral, neutron-positive, proton-negative
1. Which subatomic particles are paired with their charges?
A) Cr B) Cu C) Ni D) Se
2. In the ground state, an atom of which element has twovalence electrons?
A) absorb energyB) absorb positrons
C) emit energyD) emit positrons
3. The atoms in a sample of an element are in excitedstates. A bright-line spectrum is produced when theseatoms
A) Positrons are located in shells outside the nucleus.B) Neutrons are located in shells outside the nucleus.C) Protons are located in orbitals outside the nucleus.D) Electrons are located in orbitals outside the nucleus.
4. Which statement describes a concept included in thewave-mechanical model of the atom?
A) atomic massB) molar massC) number of neutrons per atomD) number of protons per atom
5. All elements on the modern Periodic Table are arrangedin order of increasing
A) ammoniaB) chlorine
C) neonD) nitrogen
6. At STP, which substance is a noble gas?
A) different molecular structures and differentproperties
B) different molecular structures and the sameproperties
C) the same molecular structure and differentproperties
D) the same molecular structure and the sameproperties
7. At STP, oxygen exists in two forms, and .These two forms of oxygen have
A) decompositionB) distillation
C) sublimationD) vaporization
8. Which term identifies a type of chemical reaction?
A) Sodium has a melting point of 371 K.B) Sodium has a molar mass of 23 grams.C) Sodium can conduct electricity in the liquid phase.D) Sodium can combine with chlorine to produce a
salt.
9. Which statement describes a chemical property ofsodium?
A) poloniumB) sulfur
C) seleniumD) tellurium
10. Based on Table S, an atom of which element has the weakest attraction for electrons in achemical bond?
A) Energy is absorbed as a bond is formed.B) Energy is absorbed as a bond is broken.C) Energy is released as a bond is formed.D) Energy is released as a bond is broken.
11. Given the balanced equation:
Which statement describes what occurs during thisreaction?
A) O and SeB) O and Sr
C) O and HD) O and P
12. Which atoms will bond when valence electrons aretransferred from one atom to the other?
A)B)
C)D)
13. Which sample of matter is a mixture?
A) increase the energy content of the gas sampleB) produce strong attractive forces between the gas
particlesC) result in a net loss of energy by the gas sampleD) transfer energy between the gas particles
14. According to kinetic molecular theory, collisionsbetween gas particles in a sample of an ideal gas
A) ethaneB) propanone
C) siliconD) water
15. Which substance can not be broken down by achemical change?
A) B) C) D)
16. Which particle has two neutrons?
A) average potential energy of the particles of thesample
B) average kinetic energy of the particles of thesample
C) total nuclear energy of the sampleD) total thermal energy of the sample
17. The temperature of a sample of matter is a measure ofthe
A) 37 K and 1 atmB) 37 K and 8 atm
C) 347 K and 1 atmD) 347 K and 8 atm
18. Under which conditions of temperature and pressuredoes a real gas behave most like an ideal gas?
A) a compoundB) an element
C) a mixtureD) a substance
19. The ratio of chromium to iron to carbon varies amongthe different types of stainless steel. Therefore, stainlesssteel is classified as
A) protons lostB) neutrons lost
C) neutrons gainedD) electrons gained
20. In a redox reaction, the number of electrons lost isequal to the number of
A) a longer half-life and the same decay modeB) a longer half-life and a different decay modeC) a shorter half-life and the same decay modeD) a shorter half-life and a different decay mode
21. Compared to the half-life and decay mode of thenuclide , the nuclide has
A) Ionic bonds are broken.B) Ionic bonds are formed.C) Energy is converted to mass.D) Mass is converted to energy.
22. Which net change occurs in a nuclear fusion reaction?
A) An atom is electrically neutral.B) An atom is mostly empty space.C) The nucleus of an atom is negatively charged.D) The electrons in an atom are located in specific
shells.
23. Which conclusion was drawn from the results of thegold foil experiment?
A) 2-7-3 B) 2-7-6 C) 2-8-2 D) 2-8-5
24. Which electron configuration represents an atom ofmagnesium in an excited state?
A) Group 1B) Group 2
C) Group 17D) Group 18
25. Which group on the Periodic Table has elements withatoms that tend not to bond with atoms of otherelements?
A) 1 B) 2 C) 17 D) 18
26. Which group on the Periodic Table has at least oneelement in each of the three phases of matter at STP?
A) one electron in the outermost shellB) two electrons in the outermost shellC) one neutron in the nucleusD) two neutrons in the nucleus
27. Rubidium and cesium have similar chemical propertiesbecause, in the ground state, the atoms of both elementseach have
A) decreasesB) increasesC) decreases, then increasesD) increases, then decreases
28. As the first five elements in Group 15 are considered inorder of increasing atomic number, first ionizationenergy
A) B) C) D)
29. Which ion in the ground state has the same electronconfiguration as an atom of argon in the ground state?
A) Evaporate the water, then filter out the salt.B) Evaporate the water, then filter out the sand.C) Filter out the salt, then evaporate the water.D) Filter out the sand, then evaporate the water.
30. A mixture consists of sand and an aqueous salt solution.Which procedure can be used to separate the sand, salt,and water from each other?
A) 1.0 atmB) 2.0 atm
C) 3.0 atmD) 4.0 atm
31. A sample of hydrogen gas at 2.0 atmospheres and 273K occupies a volume of 5.0 liters. The gas sample iscompletely transferred to a 10.0-liter sealed, rigidcontainer. What is the new pressure of the gas samplewhen the temperature returns to 273 K?
A) HF B) HCl C) HBr D) HI
32. Which substance in the table below has the strongest intermolecular forces?
A)B)C)D)
33. Which equation represents a spontaneoustransmutation?
34. Determine the vapor pressure of ethanol at .
35. A student drew the Lewis electron-dot diagram below to represent sodium chloride .
Explain why this diagram is not an accurate representation for the bonding in NaCl
36. Given the formula for heptanal:
Determine the gram-formula mass of heptanal.
37. Compare the mass of a proton to the mass of an electron.
38. In nature, 1.07% of the atoms in a carbon sample are C-13 atoms. Show a numerical setup for calculatingthe number of C-13 atoms in a sample containing atoms of carbon.
39. Base your answer to the following question on information below and on your knowledge of chemistry.
A sample of nitric acid contains both ions and ions. This sample has a pH value of 1.Write a name of the positive ion present in this sample.
Base your answers to questions 40 and 41 on the information below and on your knowledge of chemistry.
A sample of a substance is a liquid at 65°C. The sample is heated uniformly to 125°C. The heatingcurve for the sample at standard pressure is shown below.
40. Determine the boiling point of the sample at standard pressure.
41. State what happens to the potential energy of the particles of the sample during time interval BC.
Base your answers to questions 42 through 45 on the information below and on your knowledge ofchemistry.
One fission reaction for U-235 is represented by the balanced nuclear equation below.
Both radioisotopes produced by this fission reaction undergo beta decay. The half-life of Xe-140 is13.6 seconds and the half-life of Sr-94 is 1.25 minutes.
42. Explain, in terms of both reactants and products, why the reaction represented by the nuclear equation is afission reaction.
43. Complete the equation below for the decay of Xe-140 by writing a notation for the missing product.
44. Determine the time required for an original 24.0-gram sample of Sr-94 to decay until only 1.5 grams of thesample remains unchanged.
45. On the diagram, draw an arrow to represent the path of an emitted beta particle in the electric field betweentwo oppositely charged metal plates.
46. Base your answer to the following question on the information below and on your knowledge of chemistry.
In a laboratory investigation, a solution that contains 13.2 grams of reacts completely witha solution that contains 12.0 grams of NaI, producing 18.4 grams of and an undetermined mass ofa second product, . This reaction is represented by the balanced equation below.
Determine the mass of produced.
Base your answers to questions 47 through 49 on information below and on your knowledge of chemistry.
The two naturally occurring isotopes of antimony are Sb-121 and Sb-123. The table below shows theatomic mass and percent natural abundance for these isotopes.
Antimony and sulfur are both found in the mineral stibnite, . To obtain antimony, stibnite isroasted (heated in air), producing oxides of antimony and sulfur. The unbalanced equation belowrepresents one of the reactions that occurs during the roasting.
47. Determine the percent composition by mass of antimony in stibnite (gram-formula mass = 340. g/mol).
48. Show a correct numerical setup for calculating the atomic mass of antimony.
49. Complete the balancing of the equation below for the roasting of stibnite, using the smallest whole-numbercoefficients.
50. Base your answer to the following question on the information below and on your knowledge of chemistry.
In a laboratory investigation, ammonium chloride was dissolved in water. Laboratory proceduresand corresponding observations made by a student during the investigation are shown in the tablebelow.
State evidence from the investigation that indicates the process of dissolving the NH4Cl in water isendothermic.
51. Base your answer to the following question on the information below and on your knowledge of chemistry.
Coal is a fuel consisting primarily of carbon. In an open system, the carbon that burns completely inair produces carbon dioxide and heat. This reaction is represented by the balanced equation below.
Use the key to draw at least five particles in the box to represent the phase of the product.
