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Chem > Chapter 3&4 > Flashcards

Chapter 3&4 Flashcards

0
Q

What is used to represent an element?

A

Unique Symbol

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1
Q

Who is credited for the most current version of the periodic table?

A

Mendeleev

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2
Q

What are used to represent compounds?

A

Formulas

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3
Q

What are some of the symbols based on?

A

Latin or German name of the element

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4
Q

What are the rows and columns of the periodic table called?

A

Periods and Groups

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5
Q

What are the elements in the A Groups called?

A

Representative Elements

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6
Q

What are the elements in the B group called?

A

Transition Elements

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7
Q

What group is the alkali metals?

A

Group 1A

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8
Q

What group is the alkaline Earth metals?

A

Group 2A

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9
Q

What group are the halogens?

A

Group 7A

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10
Q

What group are the noble gases?

A

Group 8A

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11
Q

What is the atomic number?

A

Number of protons in the nucleus

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12
Q

How do you determine the number of electrons in a neutral atom?

A

They are the same number as the protons

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13
Q

How do you determine the mass number?

A

Protons+Neutrons

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14
Q

What is an isotope?

A

Atoms that have the same number of protons but different numbers of neutrons. They have the same atomic mass but different mass numbers.

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15
Q

Calculate an isotope?

A

Abundance(Atomic Mass)+x+x then divide by 100

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16
Q

What is light?

A

Electromagnetic radiation that oscillates along as a wave.

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17
Q

What are the three variables that describe wave properties?

A

Wave length, frequency, and amplitude

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18
Q

What is the formula for frequency, cycles per second?

A

V= c/wavelength

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19
Q

What is a continuous spectrum?

A

When white light is passed through a prism. Contains all wavelengths of visible light

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20
Q

What is a line spectrum?

A

Each line corresponds to a discrete wavelength.

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21
Q

What is Rygbergs equation?

A

-91.2051795273021/(1/n2 final)-1/n2 initial)

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22
Q

What is planks constant?

A

H=6.62608x10^8

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23
Q

What is Einstein’s famous equation?

A

E=mc^2

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24
Q

What are the electrons attracted to the nucleus by?

A

Electrical Force

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25
Q

What is the photoelectric effect classical method?

A

Increase energy by increasing amplitude but nothing happened. Increase frequency enough an electron is emitted

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26
Q

What were the results of the photoelectric effect?

A

Light acts like a particle. Energy must overcome the binding energy of the electron to the nucleus. E=hv E=(hc)/wavelength

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27
Q

What did DeBroglie propose?

A

A photon not only carries energy but also carries momentum.
Momentum is p=mv
Energy and momentum are inversely proportional to wavelength.

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28
Q

What is the Compton effect?

A

Put X-rays on matter and measure the scattered radiation. Scattered X-ray didn’t have same wavelength so photons are particles.

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29
Q

What is the wave theory?

A

X-ray should transfer some of its energy to the electron and emerge with a lower energy. Wavelength 2 equals wavelength 1

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30
Q

What is the particle theory?

A

X-ray should transfer its energy to the electron. Wavelength 2 > wavelength 1

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31
Q

Is light a wave or particle?

A

Has both wave and particle properties.

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32
Q

What is heisenbergs uncertainty principle?

A

Limitation to just how precisely we know both the position and momentum of a particle at a given time.

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33
Q

What is heisenbergs formula?

A

Formula

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34
Q

How are the locations and energy of electrons specified?

A

Shell, subshell, and orbital

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35
Q

What is an orbital?

A

Wave function.

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36
Q

What is probability distribution?

A

Intensity of color is used to indicate the probability value near a given point in space

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37
Q

Hydrogen 1s orbital

A

Encloses 90% of the total electron probability

38
Q

Principle(n)

A

Size and energy of the orbital

39
Q

Angular(l)

A

Shape of atomic orbitals(sometimes called a subshell)

40
Q

Magnetic(m)

A

Orientation of the orbital in space relative to the other orbitals in the atom +/-

41
Q

Electron spin(ms)

A

Can be +1/2 or -1/2

42
Q

Principle. What is the value of n?

A

The periods. 1,2,3,4, etc.

43
Q

Angular. What are the subshells?

A

S,p,d, or f

44
Q

What does the s orbital look like?

A

Sphere. Single s orbital

45
Q

What does the p orbital look like?

A

Peanut. 3 p orbitals.

46
Q

What does the d orbital?

A

Daisy. 5 d orbitals.

47
Q

What does the f orbital look like?

A

Complex flower. 7 f orbitals.

48
Q

Total number of electrons in the subshells

A

S 2
P 6
D 10
F 14

49
Q

What is the aufbau principle?

A

Protons are added one by one to the nucleus to build up elements. Electrons prefer orbitals in the order of s,p,d, and then f.

50
Q

What is the penetration effect?

A

A 2s electron penetrates to the nucleus more than a 2p orbital. This causes a 2s orbital to be attracted to the nucleus more strongly. 2s is lower in energy.

51
Q

What is hunds rule?

A

Electrons will not join other electrons in a orbital of a subshell if an empty orbital of the same energy is available. More unpaired electrons=lower in energy

52
Q

What is the Pauli Exclusion Principle?

A

Electrons behave as if they spin on axis. Only electrons spinning in opposite directions can occupy the same orbital within a subshell.

53
Q

What happens to the electron configuration if it has a charge?

A

Positive- subtract electrons

Negative- add electrons

54
Q

Valence shell?

A

Shell that contains the outermost electrons. Atoms with the same number of electrons in the outer shell have similar chem properties.

55
Q

Noble gas configuration?

A

Write down lowest atomic number noble gas closest to the given element. Continue with normal electron configuration.

56
Q

Metallic properties?

A

High thermal and electric conductivity.
Ductility (plastically deformed without fracture)
Malleability and metallic luster

57
Q

Metalloid properties

A

Has properties between those of metal and nonmetals. Exhibits characteristics properties of each type.

58
Q

Nonmetallic properties.

A

Opposite of metal properties. Occur as brittle, powdery solids or gases.

59
Q

Electro negativity.

A

A measure of the tendency of an atom to attract a bonding pair of electrons. Uses Pauling scale.
Fluorine is most electronegative. Cesium and francium is the least.

60
Q

Atomic radii

A

Farther toward the left the bigger it is. Negative atoms are larger.

61
Q

Ionization energy?

A

Energy required to remove an electron from a gaseous atom or ion. Down a group energy deceased. Same as electro negativity.

62
Q

Electron affinity.

A

Energy change associated with the addition of an electron to a gaseous atom. Across a period = more negative. Down a group = more positive less exothermic.

63
Q

Chemical rxn involve _____ on energy.
Breaking bonds ____ energy.
Forming bonds ____ energy.

A

Changes
Requires
Releases

64
Q

What is thermochemistry?

A

Study of changes in energy in chem rxn.

Energy= measurable value

65
Q

What is temperature?

A

Measures the average molecular motions in a system.

66
Q

What is heat?

A

Amount of energy in a system.

67
Q

What are the differences between heat and temperature?

A

Different units

Heat can be transported without changing the temperature of a substance (latent heat)

68
Q

How are temp and heat related?

A

As Heat goes up temp goes up

69
Q

What is energy?

A

Capacity to do work or produce heat.

70
Q

What is work?

A

Force acting over a distance.

71
Q

What is the law of conservation of energy?

A

Energy can be converted from one form to another but can’t be created or destroyed.
Total energy in universe is constant.
First law of thermodynamics.

72
Q

What is the difference between energy and work, heat?

A

Energy is a state function work an get aren’t.

73
Q

What are the two types of energy reactions?

A

Exothermic and endothermic

74
Q

What is exothermic reaction?

A

Release heat as a product.

Combustion of a log in a fireplace.

75
Q

What is endothermic reaction?

A

Absorb heat as a product.

Ice melting.

76
Q

What are the two types of energy?

A

Kinetic and potential.

77
Q

What is kinetic?

A 
Energy of motion. 
KE=1/2mv^2
Defines temp. 
Particles vibrating. Fast= hot
                              Slow= cold
78
Q

What is potential energy?

A

Stored energy

79
Q

To change internal energy of a system

A

E= q+w

80
Q

Endothermic heat is

A

Gained and positive

81
Q

Exothermic heat is

A

Lost and negative

82
Q

Work formula

A

W=-P¥V
P x A x h = p¥v
¥= triangle

83
Q

What is calorimeter?

A

Science of measuring heat.

84
Q

What is the amount of heat required to raise the temperature of 1g of a substance?

A

1 degrees Celsius

85
Q

What are the two types of molar heat?

A

Vaporization

Fusion

86
Q

What is the molar heat of vaporization?

A

Amount of heat needed to change one mole of liquid into one mole of gas at its boiling point.

87
Q

What is a nonvolatile liquid?

A

A liquid that evaporates slowly.

88
Q

What is a volatile liquid?

A

A liquid that evaporates quickly.

89
Q

What is molar heat of fusion?

A

Amount of heat needed to change one mole of solid into one mole of liquid at its melting point.

90
Q

Molar heat capacity?

A

Amount of heat necessary to raise the temp of one mole of a substance by one degree Celsius.

91
Q

Temp equation

A

Final temp - initial temp

92
Q

What is enthalpy?

A

State function.

The energy used or produced in a chemical reaction

93
Q

What is Hess’s law?

A

Going from a set of reactants to a se of products. The change in enthalpy is the same whether the reaction takes place in 1 step or in a series of steps.

Chem (5 decks)

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