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Chemistry Final > Chemistry Final > Flashcards

Chemistry Final Flashcards

1
Q

The chemical bonds of a water molecule are:

a) Ionic
b) Covalent
c) Polar Covalent
d) Hydrogen bonds
e) none of the above

A

b) Covalent

c) Polar Covalent

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2
Q

The sequence of elements (which element comes after a given element) on the Periodic Table is based on :

a) Atomic mass of each element
b) Number of neutrons in the atom of each element
c) Number of protons in the atom of each element
d) Number of electrons in the atom of each element
e) none of the above

A

c) Number of protons in the atom of each element

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3
Q

How many bonds exist between two atoms of oxygen to make one molecule of oxygen gas?

a) 0
b) 1
c) 2
d) 3
e) none of the above

A

c) 2

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4
Q

How many electrons are in the outer shell of Bismuth (Bi)?

a) 1
b) 3
c) 5
d) 7
e) 8

A

c) 5

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5
Q

What is another name for the rows on the Periodic Table?

a) Groups
b) Lines
c) Series
d) Periods
e) None of the above

A

d) Periods

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6
Q

What is the max number of electrons the 5th electron shell of an atom can hold?

a) 8
b) 18
c) 32
d) 50
e) 72

A

d) 50

2n^2= 2(5)^2=50

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7
Q

What is the charge on the metal ion of Fe2S3?

a) -3
b) +3
c) -2
d) +2
e) none of the above

A

b) +3

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8
Q

The correctly rounded answer to the calculation (1.45 x 0.03515) is:

a) 0.051
b) 0.05097
c) 0.05
d) 0.0510
e) 0.0509675

A

d) 0.0510

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9
Q

In scientific notation the number 0.0030600 is correctly expressed as

a) 3.0600 x 10^-2
b) 0.30600 x 10^-2
c) 0.306 x 10^-2
d) 3.06 x 10^-3
e) 3.0600 x 10^-3

A

e) 3.0600 x 10^-3

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10
Q

One sample of CaC2 contains 0.150 mol. of carbon. How many grams of calcium are also in the sample?

a) 1.50 g Ca
b) 3.01 g Ca
c) 5.1 g Ca
d) 0.30 g Ca
e) none of the above

A

b) 3.01 g Ca

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11
Q

How many moles are there in a 25.0 mg sample of calcium carbonate (CaCO3)?

a) 0.250 moles
b) 0. 0550 moles
c) 0.00250 moles
d) 0.000250 moles
e) none of the above

A

d) 0.000250 moles

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12
Q

What is the formula for the compound that will form with lithium and nitrogen?

a) LiN
b) Li2N
c) Li3N
d) LiN2
e) LiN3

A

c) Li3N

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13
Q

Name the compound Fe2(CO3)3

a) Ferrous carbonate
b) Iron tricarbonate
c) Diiron tricarbonate
d) Iron (III) carbonate
e) none of the above

A

d) Iron (III) carbonate

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14
Q

How many protons (p+) and electrons (e-) are in a K+ ion?

a) 19p and 19 e
b) 20 p and 20 e
c) 19 p and 20 e
d) 19 p and 18 e
e) 20 p and 21 e

A

d) 19 p and 18 e

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15
Q

How many protons, neutrons and electrons are in a U-235 atom?

a) 92 p, 92 n, 92 e
b) 235 p, 235 n, 235 e
c) 92 p, 235 n, 92 e
d) 92 p, 143 n, 92 e
e) 143 p, 92 n, 92 e

A

d) 92 p, 143 n, 92 e

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16
Q

If a can contains 22.0 oz of soup, how many grams of soup is that? (1lb=16 oz, 1lb= 454 g)

a) 330 g
b) 20.6 g
c) 523 g
d) 624 g
e) 0,775 g

A

d) 624 g

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17
Q

The wavelength of a red laser pointer is 650 nm. How long is the wavelength in meters?

a) 6.50 x 10^7m
b) 6.50 x 10^9m
c) 6.50 x 10^-7m
d) 6.50 x 10^-9m
e) none of the above

A

c) 6.50 x 10^-7m

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18
Q

How many atoms of hydrogen are in the molecule: (NH4)2HPO4?

a) 2
b) 4
c) 8
d) 9
e) none of the above

A

d) 9

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19
Q

Which of the following pairs of elements are likely to form an ionic compound?

a) Helium and oxygen
b) Chlorine and bromine
c) Magnesium and Chlorine
d) Sodium and potassium
e) none of the above

A

c) Magnesium and Chlorine

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20
Q

How many protons and electrons are in Sr+2?

a) 36 protons, 36 electrons
b) 38 protons, 38 electrons
c) 38 protons, 36 electrons
d) 38 protons, 40 electrons
e) none of the above

A

c) 38 protons, 36 electrons

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21
Q

The mass number of an element is?

a) the number of protons
b) the number of protons and electrons
c) the number of protons and neutrons
d) the weighted average of all isotopes of the element
e) none of the above

A

c) the number of protons and neutrons

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22
Q

The most abundant isotope of iron is 56Fe. How many protons does this isotope have?

a) 56
b) 30
c) 26
d) 55.85
e) none of the above

A

c) 26

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23
Q

A neutron carries a charge of

a) +1
b) -1
c) +2
d) -2
e) Zero

A

e) Zero

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24
Q

Mg gives up 2 electrons to oxygen to form Mg ion and oxygen ion. What is the change in the atomic number of magnesium?

a) +1
b) -1
c) +2
d) -2
e) zero

A

e) zero

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25
Q

Ethyl alcohol has a density of 0.79 g/mL. what is the mass of 53 mL of ethyl alcohol?

a) 67 g
b) 42 g
c) 5.3 g
d) 79 g
e) 0.015 g

A

b) 42 g

26
Q

How many protons are present in 239Pu
94

a) 94
b) 150
c) 244
d) 338
e) none of the above

A

a) 94

27
Q

How many neutrons are present in 239Pu
94

a) 94
b) 145
c) 244
d) 338
e) none of the above

A

b) 145

28
Q

Which of the following is an isotope of 239Pu
94

a) 245X
    94
b) 245X
    95
c) 244X
    95
d) 244X
    93
e) none of the above
A

a) 245X

94

29
Q

What period on the periodic table is Plutonium in?

a) 2
b) 5
c) 6
d) 7
e) none of the above

A

d) 7

30
Q

Name this Compound Pu2(SO4)3?

a) Plutonium sulfate
b) Plutonium (II) sulfate
c) Plutonium (III) sulfate
d) Plutonium (IV) sulfate
e) none of the above

A

c) Plutonium (III) sulfate

31
Q

The empirical formula for a compound is NaS2O3 and its molecular weight is 270.4g/mole. What is its molecular formula?

a) NaS2O3
b) Na2S4O6
c) Na3S6O9
d) Na4S8O12
e) none of the above

A

b) Na2S4O6

32
Q

The molar ratio of carbon to hydrogen in glucose C6H12O6 is

a) 6 to 1
b) 1 to 2
c) 2 to 1
d) 1 to 6
e) none of the above

A

b) 1 to 2

33
Q

How many moles of oxygen are needed to complete consume heptane in the following reaction? C7H16+O2 –> CO2 + H2O

a) 6
b) 9
c) 11
d) 22
e) none of the above

A

c) 11

C7H16 +11O2 –> 7CO2 + 8H2O

34
Q

The constant number 6.023 x 10^23 is a result of

a) the natural laws of the universe
b) the fact that 1.00 amu is equal to 1.66 x 10^-24g
c) the fact that all molecules contain that number of atoms
d) the fact that molecular mass cannot be directly calculated
e) none of the above

A

b) the fact that 1.00 amu is equal to 1.66 x 10^-24g

35
Q

The constant number 6.02 x 10^23 is known as

a) Boyle’s Law
b) Gibb’s number
c) dalton’s number
d) avogrado’s number
e) none of the above

A

d) Avogrado’s Number

36
Q

How many moles of Fe are in 2.75 moles of Fe3O4?

a) 2.75
b) 5.50
c) 8.25
d) 11.00
e) none of the above

A

c) 8.25

37
Q

How many moles of oxygen are in Ca3(PO4)2?

a) 1
b) 4
c) 6
d) 8
e) none of the above

A

d) 8

38
Q

How many moles of water in Calcium sulfate dihydrate?

a) zero
b) 1
c) 2
d) 4
e) none of the above

A

c) 2

39
Q

6.02 x 10^23 of anything is known as a

a) squirrel
b) standard molar equivalent
c) standard molar mass
d) mole
e) none of the above

A

d) mole

40
Q

What is the empirical formula for magnesium phosphate?

a) MgPO4
b) Mg3(PO4)2
c) Mg2(PO4)3
d) Mg2PO4
e) none of the above

A

b) Mg3(PO4)2

41
Q

Which of the following is NOT a condition for the Kinetic-Molecular theory?

a) Gases are composed of small particles that move rapidly and randomly
b) Any attractive forces between gas particles are ignored
c) The volume of a gas molecule is insignificant compared to the total volume of the gas
d) Average kinetic energy of a population of gas particles is proportional to Fahrenheit temperatures
e) Gas particles move in a straight line until they collide with something

A

d) Average kinetic energy of a population of gas particles is proportional to Fahrenheit temperatures

42
Q

That pressure is inversely proportional to volume is ___________ law?

a) Boyles
b) Charles’
c) Gay-Lussac’s
d) Avogadro’s
e) None of the above

A

a) Boyles

43
Q

A device used to measure atmospheric pressure is called

a) open ended manometer
b) closed ended manometer
c) Atmospheric manometer
d) Barometer
e) none of the above

A

d) barometer

44
Q

Which of the following gas samples would be most likely to behave ideally under the stated conditions?

a) Ne at STP (standard Temperature and pressure)
b) CO at 200 atm and 25K
c) SO2 at 20 at and 0K
d) N2 at 1 atm and -70C
e) O2 at 400 atm and 25C

A

a) Ne at STP

45
Q

When a substance is surrounded by water molecules such as in a solution of sodium chloride or sugar, it is said to be:

a) ionized
b) dissociated
c) hydrated
d) electrolyzed
e) none of the above

A

c) hydrated

46
Q

As part of the scientific method, hypotheses are always based on

a) laws
b) theories
c) experiments
d) observation
e) none of the above

A

d) observations

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47
Q

A scientific hypothesis must be

a) testable
b) always true
c) based on experimental results
d) all of the above
e) none of the above

A

a) testable

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48
Q

As pressure is increased the volume of a sample of gas decreases lineraly at constant temperature. is an example of

a) a theory
b) a hypothesis
c) a law
d) experimental data
e) experimental procedure

A

c) a law

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49
Q

Chose the types of intermolecular attractive forces (dipole-dipole, london, hydrogen bonding, etc) that are present in HF

a) dipole-dipole
b) H-bonding
c) london forces
d) all of the above
e) none of the above

A

d) all of the above

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50
Q

What is the strongest intermolecular force exhibited in a carbon dioxide molecule

a) hydrogen bonding
b) london forces
c) dipole-dipole forces
d) ion-dipole
e) none of the above

A

b) london forces

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51
Q

The direction water will flow through a semi-permeable membrane if the concentration of solute on one side of the membrane is lower than the other side is _________

a) toward the lower solute concentration
b) depends on the characteristics of the membrane
c) water, being the solvent, is saturated on both sides of the membrane
d) toward the higher solute concentration
e) none of the above

A

d) toward the higher solute concentration

52
Q

The process of water molecules surrounding and separation ions is known as

a) surrounding
b) ionization
c) hydration
d) dehydration
e) none of the above

A

c) hydration

53
Q

the force that causes nonpolar solutes to dissolve into nonpolar solvents is called

a) hydration
b) entropy
c) effusion
d) brownian motion
e) none of the above

A

b) entropy

54
Q

The amount of solute in a given amount of solvent or solution is called

a) solubility
b) concentration
c) molar solubility
d) mass
e) none of the above

A

b) concentration

55
Q

If a solution becomes more concentrated its osmotic pressure

a) increases
b) decreases
c) stays the same
d) both increases at first then decreases
e) none of the above

A

a) increases

56
Q

Gas concentrations tend to ______ with increasing gas pressure

a) increase
b) decrease
c) stay the same
d) increase then decrease
e) none of the above

A

a) increase

57
Q

Physical properties of solutions that depend mostly on the relative populations of particles in the solutions and not on their chemical identities are called________

a) solution properties
b) ideal solution properties
c) colligative properties
d) solubility properties
e) none of the above

A

c) colligative properties

58
Q

When the mole fraction of the solvent is equal to 1, the vapor pressure of the solution is ________

a) infinite
b) insignificant
c) equal to the vapor pressure of the solvent
d) equal to one
e) none of the above

A

c) equal to the vapor pressure of the solvent

59
Q

Raoult’s Law states_______________________

a) vapor pressure of one component equals vapor pressure of solution
b) vapor pressure of all components equals vapor pressure of solution
c) vapor pressure of solution is proportional to the mole fraction of the components
d) vapor pressure of a solution is a function of the mole fraction of the components and their vapor pressures
e) none of the above

A

d) vapor pressure of solution is a function of the mole fraction of the components and their vapor pressures

60
Q

A mixture of 1.0 mol He and 1.0 mol Ne are at STP in a rigid container. which of the following statements is true?

a) one gas has half the pressure of the other gas
b) both gases contribute to the density of the mixture under these conditions
c) molecules of both gases contain the same amount of energy
d) the mixture has a total volume of 22.4 L
e) none of the above

A

c) molecules of both gases contain the same amount of energy

Chemistry Final (1 decks)

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