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1.Compared to the charge of a proton, the charge of an electron has (1) a greater magnitude and the same sign (2) a greater magnitude and the opposite sign (3) the same magnitude and the same sign (4) the same magnitude and the opposite sign 2. Which atom has the largest atomic radius? (1) potassium (3) francium (2) rubidium (4) cesium 3. In the wave-mechanical model of the atom, an orbital is defined as (1) a region of the most probable proton location (2) a region of the most probable electron location (3) a circular path traveled by a proton around the nucleus (4) a circular path traveled by an electron around the nucleus 4. When an excited electron in an atom moves to the ground state, the electron (1) absorbs energy as it moves to a higher energy state (2) absorbs energy as it moves to a lower energy state (3) emits energy as it moves to a higher energy state (4) emits energy as it moves to a lower energy State 5. The atomic mass of magnesium is the weighted average of the atomic masses of (1) all of the artificially produced isotopes of Mg (2) all of the naturally occurring isotopes of Mg (3) the two most abundant artificially produced isotopes of Mg (4) the two most abundant naturally occurring isotopes of Mg

6. Which sample of copper has atoms with the lowest average kinetic energy? (1) 10. g at 45°C (3) 30. g at 25°C (2) 20. g at 35°C (4) 40. g at 15°C 7. Which change results in the formation of different substances? (1) burning of propane (2) melting of NaCl(s) (3) deposition of CO2(g) (4) solidification of water 8. Which substance can not be broken down by a chemical change? (1) ammonia (3) propanal (2) ethanol (4) zirconium 9. Which element is a liquid at STP? (1) bromine (3) francium (2) cesium (4) iodine 10. What is the number of electrons in a completely filled second shell of an atom? (1) 32 (3) 18 (2) 2 (4) 8 11. What is the number of electrons in an atom that has 3 protons and 4 neutrons? (1) 1 (3) 3 (2) 7 (4) 4 12. As a result of the gold foil experiment, it was concluded that an atom (1) contains protons, neutrons, and electrons (2) contains a small, dense nucleus (3) has positrons and orbitals (4) is a hard, indivisible sphere 13. Which particle has the least mass? (1) alpha particle (3) neutron (2) beta particle (4) proton

14. The elements in Group 2 are classified as (1) metals (3) nonmetals (2) metalloids (4) noble gases 15. Which pair represents two forms of an element in the same phase at STP but with different structures and different properties? (1) I2(s) and I2(g) (3) H2(g) and Hg(g) (2) O2(g) and O3(g) (4) H2O(s) and H2O(ℓ) 16. The elements on the Periodic Table are arranged in order of increasing (1) atomic mass (3) molar mass (2) atomic number (4) oxidation number 17. Which sample of CO2 has a definite shape and a definite volume? (1) CO2(aq) (3) CO2(ℓ) (2) CO2(g) (4) CO2(s) 18. Which statement describes the particles of an ideal gas according to the kinetic molecular theory? (1) The gas particles are arranged in a regular geometric pattern. (2) The gas particles are in random, constant, straight-line motion. (3) The gas particles are separated by very small distances, relative to their sizes. (4) The gas particles are strongly attracted to each other.

Yellow: 1. A solid element that is malleable, a good conductor of electricity, and reacts with oxygen is classified as a (1) metal (3) noble gas (2) metalloid (4) nonmetal 2. Three forms of energy are (1) chemical, exothermic, and temperature (2) chemical, thermal, and electromagnetic (3) electrical, nuclear, and temperature (4) electrical, mechanical, and endothermic

3. Which quantity can vary among atoms of the same element? (1) mass number (2) atomic number (3) number of protons (4) number of electrons

4. A sample of CO2(s) and a sample of CO2(g) differ in their (1) chemical compositions (2) empirical formulas (3) molecular structures (4) physical properties

5. Which equation represents sublimation? (1) Hg(ℓ) → Hg(s) (3) NH3(g) → NH3(ℓ) (2) H2O(s) → H2O(g) (4) CH4(ℓ) → CH4(g)

6. Which statement describes the particles of an ideal gas, based on the kinetic molecular theory? (1) The motion of the gas particles is orderly and circular. (2) The gas particles have no attractive forces between them. (3) The gas particles are larger than the distances separating them. (4) As the gas particles collide, the total energy of the system decreases.

7. Two grams of potassium chloride are completely dissolved in a sample of water in a beaker. This solution is classified as (1) an element (2) a compound (3) a homogeneous mixture (4) a heterogeneous mixture

8. Powdered sulfur is yellow, and powdered iron is gray. When powdered sulfur and powdered iron are mixed at 20°C, the powdered iron (1) becomes yellow (3) remains ionic (2) becomes a liquid (4) remains magnetic

9. What is the approximate mass of a proton? (1) 1 u (3) 1 g (2) 0.0005 u (4) 0.0005 g 10. 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 stat

11. Which particle has no charge? (1) electron (3) positron (2) neutron (4) proton

12. 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

13. The element sulfur is classified as a (1) metal (3) nonmetal (2) metalloid (4) noble gas

14. 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

15. 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

16. 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 17. Which property is a measure of the average kinetic energy of the particles in a sample of matter? (1) mass (3) pressure (2) density (4) temperature 18. 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.

Blue: 1. A mixture of sand and table salt can be separated by filtration because the substances in the mixture differ in (1) boiling point (3) freezing point (2) density at STP (4) solubility in water 2. 25 In the wave-mechanical model of the atom, an orbital is the most probable location of (1) a proton (3) a neutron (2) a positron (4) an electron 3. The mass of a proton is approximately equal to the mass of (1) an alpha particle (3) a positron (2) a beta particle (4) a neutron 4. What must occur when an electron in an atom returns from a higher energy state to a lower energy state? (1) A specific amount of energy is released. (2) A random amount of energy is released. (3) The atom undergoes transmutation. (4) The atom spontaneously decays. 5. At STP, which physical property of aluminum always remains the same from sample to sample? (1) mass (3) length (2) density (4) volume 6. Which statement describes a chemical property of silicon? (1) Silicon has a blue-gray color. (2) Silicon is a brittle solid at 20.°C. (3) Silicon melts at 1414°C. (4) Silicon reacts with fluorine.

7. A compound is broken down by chemical means during (1) chromatography (3) electrolysis (2) distillation (4) filtration

8. Which quantities must be conserved in all chemical reactions? (1) mass, charge, density (2) mass, charge, energy (3) charge, volume, density (4) charge, volume, energy

9. What is the charge of the nucleus of an oxygen atom? (1) 0 (3) +8 (2) -2 (4) +16 10. Every chlorine atom has (1) 7 electrons (2) 17 neutrons (3) a mass number of 35 (4) an atomic number of 17 11. Which substance can not be broken down by a chemical change? (1) ammonia (3) propane (2) methanol (4) phosphorus

12. The temperature of a sample of matter is a measure of the (1) total kinetic energy of the particles in the sample (2) total potential energy of the particles in the sample (3) average potential energy of the particles in the sample (4) average kinetic energy of the particles in the sample

13. Which unit is used to express the pressure of a gas? (1) mole (3) kelvin (2) joule (4) pascal

14. Which sample of matter sublimes at room temperature and standard pressure? (1) Br2(ℓ) (3) CO2(s) (2) Cl2(g) (4) SO2(aq)

15. Which phrase describes an atom? (1) a negatively charged nucleus surrounded by positively charged protons (2) a negatively charged nucleus surrounded by positively charged electrons (3) a positively charged nucleus surrounded by negatively charged protons (4) a positively charged nucleus surrounded by negatively charged electrons

16. An atom of lithium-7 has an equal number of (1) electrons and neutrons (2) electrons and protons (3) positrons and neutrons (4) positrons and protons

17. Which statement explains why neon is a Group 18 element? (1) Neon is a gas at STP. (2) Neon has a low melting point. (3) Neon atoms have a stable valence electron configuration. (4) Neon atoms have two electrons in the first shell.

18. A substance is classified as either an element or a (1) compound (2) solution (3) heterogeneous mixture (4) homogeneous mixture

Green: 1. Under which conditions of temperature and pressure does a real gas behave most like an ideal gas? (1) low temperature and low pressure (2) low temperature and high pressure (3) high temperature and low pressure (4) high temperature and high pressure 2. Which two gases can not be broken down by chemical means? (1) CO and He (3) Xe and He (2) CO and NH3 (4) Xe and NH3

3. Which atom in the ground state has a stable electron configuration? (1) carbon (3) neon (2) magnesium (4) oxygen

4. Which quantity is equal to one mole of Au? (1) the atomic mass in grams (2) the atomic number in grams (3) the mass of neutrons in grams (4) the number of neutrons in grams

5. Which phrase describes the molecular structure and properties of two solid forms of carbon, diamond and graphite? (1) the same molecular structures and the same properties (2) the same molecular structures and different properties (3) different molecular structures and the same properties (4) different molecular structures and different properties

6. At STP, which element is a good conductor of electricity? (1) chlorine (3) silver (2) iodine (4) sulfur

7. All phosphorus atoms have the same (1) atomic number (2) mass number (3) number of neutrons plus the number of electrons (4) number of neutrons plus the number of protons

8. A specific amount of energy is emitted when excited electrons in an atom in a sample of an element return to the ground state. This emitted energy can be used to determine the (1) mass of the sample (2) volume of the sample (3) identity of the element (4) number of moles of the element 9. Which element is paired with an excited-state electron configuration for an atom of the element? (1) Ca: 2-8-8-2 (3) K: 2-6-8-3 (2) Na: 2-8-2 (4) F: 2-8 10. An ion that consists of 7 protons, 6 neutrons, and 10 electrons has a net charge of (1) 4− (3) 3+ (2) 3− (4) 4+

11. At which temperature is the vapor pressure of ethanol equal to 80. kPa? (1) 48°C (3) 80.°C (2) 73°C (4) 101°C

12. An atom in the ground state has two electrons in its first shell and six electrons in its second shell. What is the total number of protons in the nucleus of this atom? (1) 5 (3) 7 (2) 2 (4) 8

13. A bromine atom in an excited state could have an electron configuration of (1) 2-8-18-6 (3) 2-8-17-7 (2) 2-8-18-7 (4) 2-8-17-8 14. Which electron configuration represents a selenium atom in an excited state? (1) 2-7-18-6 (3) 2-8-18-6 (2) 2-7-18-7 (4) 2-8-18-7

15. What is the overall charge of an ion that has 12 protons, 10 electrons, and 14 neutrons? (1) 2(3) 4(2) 2+ (4) 4+

16. As the elements in Period 3 are considered in order of increasing atomic number, there is a general decrease in (1) atomic mass (2) atomic radius (3) electronegativity (4) first ionization energy

17. Which electron configuration represents the electrons of a sulfur atom in an excited state? (1) 2-6-6 (3) 2-8-4 (2) 2-7-7 (4) 2-8-6

18. Which Kelvin temperature is equal to 200.°C? (1) -73 K (3) 200. K (2) 73 K (4) 473 K

Bridge cards/orange 1. Which element is a liquid at 305 K and 1.0 atmosphere? (1) magnesium (3) gallium (2) fluorine (4) iodine 2. Which list of elements consists of a metal, a metalloid, and a nonmetal? (1) Li, Na, Rb (3) Sn, Si, C (2) Cr, Mo, W (4) O, S, Te 3. What is the total amount of heat required to vaporize 1.00 gram of H2O(ℓ) at 100.°C and 1 atmosphere? (1) 4.18 J (3) 373 J (2) 334 J (4) 2260 J 4. During a flame test, a lithium salt produces a characteristic red flame. This red color is produced when electrons in excited lithium atoms (1) are lost by the atoms (2) are gained by the atoms (3) return to lower energy states within the atoms (4) move to higher energy states within the atoms 5. Compared to the energy and charge of the electrons in the first shell of a Be atom, the electrons in the second shell of this atom have (1) less energy and the same charge (2) less energy and a different charge (3) more energy and the same charge (4) more energy and a different charge 6. An atom that has 13 protons and 15 neutrons is an isotope of the element (1) nickel (3) aluminum (2) silicon (4) phosphorus

7. What is the number of electrons in an Al3+ ion? (1) 10 (3) 3 (2) 13 (4) 16 8. Which compound has the greatest percent composition by mass of sulfur? (1) BaS (3) MgS (2) CaS (4) SrS

9. What is the total number of valence electrons in a germanium atom in the ground state? (1) 22 (3) 32 (2) 2 (4) 4...