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WAZZAP > Quiz 2 > Flashcards

Quiz 2 Flashcards

1
Q
  1. The maximum number electrons that could fit in the “p” sublevel is

A. 9

B. 6

C. 3

D. 2

A

B. 6

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2
Q
  1. Element number 13 has ___ valence electrons.

A. 13

B. 10

C. 8

D. 3

A

D. 3

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3
Q
  1. Which of the following is the energy configuration for the element number 13?

A. 1s² 2s² 2p6 3s² 3p1

B. 1s² 2s² 2p6 3s1 3p1 3d1

C. 1s² 2s² 2p6 3s³

D. 1s² 2s² 2p6 3p³

A

A. 1s² 2s² 2p6 3s² 3p1

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4
Q
  1. The octet rule allows for a maximum of ____ outermost electrons in any one atom.

A. 2

B. 8

C. 16

D. there is no limit

A

B. 8

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5
Q
  1. It is a group of cation that is separated from the other groups by precipitation as chlorides.

A. alkali metal group

B. copper-arsenic group

C. aluminum-iron group

D. silver group

A

D. silver group

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6
Q
  1. It is red in acid and yellow in alkaline.

A. congo red

B. methyl orange

C. HpH

D. litmus

A

B. methyl orange

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7
Q
  1. A solution has a pH of 3.6 will give ___ color if added with a drop of thymol blue.

A. red

B. yellow

C. colorless

D. blue

A

B. yellow

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8
Q
  1. Yellowish gas

A. Cl2

B. N2

C. CO2

D. H2

A

A. Cl2

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9
Q
  1. Magnesium is obtained from

A. sea shells

B. bentonite

C. sea water

D. corals

A

C. sea water

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10
Q
  1. Methyl orange gives red color in

A. sodium carbonate solution

B. hydrochloric acid solution

C. sodium chloride solution

D. potassium hydroxide solution

A

B. hydrochloric acid solution

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11
Q
  1. The shape of a CCl4 molecule is

A. Linear

B. Trigonal planar

C. Tetrahedral

D. Bent (V-shaped)

A

C. Tetrahedral

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12
Q
  1. A double bond, such as N=N, consists of

A. One sigma bond only

B. One pi bond only

C. One sigma bond and one pi bond

D. Two pi bonds

A

C. One sigma bond and one pi bond

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13
Q
  1. Hydrogen bonds are formed between molecules when hydrogen is covalently bonded to an element that has a ______.

A. Small atomic radius and low electronegativity

B. Large atomic radius and low electronegativity

C. Small atomic radius and high electronegativity

D. Large atomic radius and high electronegativity

A

C. Small atomic radius and high electronegativity

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14
Q
  1. Deuterium is an isotope of _____.

A. hydrogen

B. oxygen

C. nitrogen

D. helium

A

A. hydrogen

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15
Q
  1. Which of the following is the lightest?

A. alpha particle

B. beta particle

C. proton

D. hydrogen

A

B. beta particle

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16
Q
  1. Which of the following is the reason that metals conduct electricity?

A. The metal atoms are close together

B. There are no empty spaces in metal structures

C. Electrons in the structure can move freely

D. Electrons and protons in the structure can move freely

A

C. Electrons in the structure can move freely

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17
Q
  1. Which of the following is a chemical change?

A. water boiling

B. natural gas burning

C. alcohol evaporating

D. ice melting

A

B. natural gas burning

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18
Q
  1. A sample of carbon dioxide that undergoes transformation from solid to liquid to gas would undergo

A. a change in density

B. a change in mass

C. a change in composition

D. no change in physical properties

A

A. a change in density

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19
Q
  1. When concentrated sulfuric acid is diluted with water, the solution becomes warm. Therefore

A. the reaction is exothermic

B. the reaction is endothermic

C. the energy of the universe is increased

D. the energy of both the system and the surroundings is decreased

A

A. the reaction is exothermic

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20
Q
  1. Which of the following has the largest atomic radius?

A. Be

B. Mg

C. Sr

D. Ba

A

D. Ba

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21
Q
  1. What is the pH of natural rain water?

A. 7.0 - 8.3

B. 2.4 – 3.4

C. 5.6 – 6.2

D. 13

A

C. 5.6 – 6.2

22
Q
  1. One sample of a solution with a pH of 10 is tested with phenolphthalein and another sample of this solution is tested with litmus. In this solution the color of the litmus is

A. blue and the phenolphthalein is pink

B. red and the phenolphthalein is pink

C. blue and the phenolphthalein is colorless

D. red and the phenolphthalein is colorless

A

A. blue and the phenolphthalein is pink

23
Q
  1. How many electrons are in the outer shell of the Na+ ion?

A. 1

B. 2

C. 3

D. 8

A

A. 1

24
Q
  1. The total number of electrons at the L shell of an atom is

A. 2

B. 8

C. 18

D. 32

A

B. 8

25
Q
  1. The total number of electrons at the fourth energy level is

A. 2

B. 8

C. 18

D. 32

A

D. 32

26
Q
  1. The mass of proton or neutron is approximately ____ times that of the electron.

A. 1,736

B. 1,900

C. 1,700

D. 1,836

A

D. 1,836

27
Q
  1. What is the maximum number of electrons in the O shell?

A. 16

B. 8

C. 32

D. 50

A

D. 50

28
Q
  1. The quantum number L signifies

A. the relative distance of the electron from the nucleus

B. the orientation in space of a particular orbital

C. the shape of an orbital

D. the spin of the electron

A

C. the shape of an orbital

29
Q
  1. What is the four set of quantum numbers of the 4s1 electron?

A. 410½

B. 410-½

C. 400-½

D. 400½

A

D. 400½

30
Q
  1. Which of the following represents an acceptable set of quantum number?

A. 2,2,-1,-1/2

B. 1,0,0,1/2

C. 5,-4,-3,1/2

D. 3,3,3,-1/2

A

B. 1,0,0,1/2

31
Q
  1. Which of the following atoms has the highest electron affinity?

A. Na

B. Cl

C. Br

D. S

A

B. Cl

32
Q
  1. The pi bond is the result of the

A. overlap of two s orbitals

B. overlap of an s orbital and a p orbital

C. overlap of two p orbitals along their axes

D. sidewise overlap of two parallel p orbitals

A

D. sidewise overlap of two parallel p orbitals

33
Q
  1. The bonding in acetylene is best described as

A. five sigma bonds

B. four sigma bonds and one pi bonds

C. five pi bonds

D. three sigma bonds and two pi bonds

A

D. three sigma bonds and two pi bonds

34
Q
  1. The conversion of sugar to ethanol and carbon dioxide with enzymes acting as catalyst is called

A. fermentation

B. polymerization

C. photosynthesis

D. digestion

A

A. fermentation

35
Q
  1. Which of the following tests is used to confirm urea?

A. Biuret test

B. Legal’s test

C. Lassaigne test

D. Wholer’s test

A

A. Biuret test

36
Q
  1. Which of the following terms describes the addition of water to the atmosphere by plants?

A. evaporation

B. condensation

C. transpiration

D. precipitation

A

C. transpiration

37
Q
  1. The pH of normal, or average , rainfall is about

A. 2.3

B. 5.7

C. 7.1

D. 8.5

A

B. 5.7

38
Q
  1. Which of the following elements does this electronic configuration represent? 1s²2s²2p5

A. F

B. C

C. N

D. Al

A

A. F

39
Q
  1. Which of the following is the strongest interaction?

A. a covalent bond

B. hydrogen bonding

C. dipole-dipole interactions

D. van der Waals

A

A. a covalent bond

40
Q
  1. Hydrophobic molecules are ______water.

A. attracted to

B. absorbed by

C. repelled by

D. mixed with

A

C. repelled by

41
Q
  1. An ideal gas differs from a real gas in that the molecules of an ideal gas _________________.

A. have no attraction for one another

B. have a molecular weight of zero

C. have appreciable molecular volume

D. have no kinetic energy

A

A. have no attraction for one another

42
Q
  1. The statement, “For a fixed mass of gas at constant temperature, gas volume is inversely proportional to gas pressure.” Is known as:

A. Avogadro’s law

B. Boyle’s law

C. Charle’s law

D. Graham’s law

A

B. Boyle’s law

43
Q
  1. If gas volume is doubled but the temperature remains constant:

A. the pressure stays the same

B. the molecules move faster

C. the kinetic energy increases

D. the molecules move slower

E. none of these answers*

A

E. none of these answers*

44
Q
  1. Subtracting the vapor pressure of water from the total pressure of a gas collected over water is an example:

A. Avogadro’s Hypothesis

B. Dalton’s law

C. Graham’s law

D. van der Waals Theory

A

B. Dalton’s law

45
Q
  1. The energy of molecules of a gas:

A. is dependent on concentration

B. is distributed over a wide range at constant temperature

C. is the same for all molecules at constant temperature

D. increases with a decrease in temperature

E. increases with an increase in pressure

A

B. is distributed over a wide range at constant temperature

46
Q
  1. Which of the following assumptions is not used to explain the ideal gas law?

A. gas particles themselves occupy a negligible percent of total gas volume

B. inter-particle forces are negligible in gases

C. collisions between gas particles are perfectly elastic

D. collisions between gas particles and container walls are perfectly elastic

E. individual gas particles are perfectly compressible to nuclear size

A

E. individual gas particles are perfectly compressible to nuclear size

47
Q
  1. If someone were to light a cigar at one end of a closed room, persons at the other end of the room might soon perceive an odor due to gaseous emissions from the cigar. Such a phenomenon is an example of:

A. monometry

B. ideality

C. effusion

D. diffusion

A

D. diffusion

48
Q
  1. The fact that a balloon filled with helium will leak more slowly than one filled with hydrogen is explained by citing:

A. Avogadro’s hypothesis

B. Dalton’s law

C. Graham’s law

D. van der Waals Theory

A

C. Graham’s law

49
Q
  1. Gases tend to behave ideally at

A. low temperature and low pressure

B. low temperature and high pressure

C. high temperature and low pressure

D. high temperature and high pressure

A

C. high temperature and low pressure

50
Q
  1. Assuming ideal gas behavior, which of the following gases would have the lowest density at standard temperature and pressure?

A. SF6

B. CF2Cl2

C. CO2

D. N2

A

D. N2

WAZZAP (31 decks)

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