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Chemistry 1 > Chemistry Exam 2 > Flashcards

Chemistry Exam 2 Flashcards

1
Q

What is light?

A

light is a wide range of energy projected by many different sources

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2
Q

What is wavelength?

A

distance between peaks

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3
Q

What is frequency?

A

cycles per second

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4
Q

What does speed of light equal?

A

speed of light= wavelength x frequency

c=(lambda)(v)

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5
Q

What is frequency directly proportional to?

A

energy

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6
Q

Is the wavelength shorter or longer when the frequency is high?

A

shorter

(the the higher the frequency, the shorter the wavelength and the higher the energy.)

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7
Q

As energy increases what happens to the frequency?

A

The frequency increases

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8
Q

What did Einstein observe?

A

He observed that when light is shined on a metal surface, electrons are produced from the surface, and the electrons emitted from the metal surface are photoelectrons. This phenomenon is called the photoelectric effect

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9
Q

What is Planck’s equation?

A

E=hv

(energy= frequency x planck’s constant)

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10
Q

Does an infrared light or ultraviolet light have more energy?

A

Ultraviolet because it is at a higher frequency, therefor higher energy.

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11
Q

How are photons created?

A

When an electron in an excited state jumps to a higher shell, and when it eventually falls back to its original shell it emits a photon

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12
Q

The further the photon falls_____?

A

the higher energy the photon will be

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13
Q

What does the Bohr model explain?

A

The Bohr model explains that electrons orbit the nucleus at fixed energy levels. Orbits further from the nucleus exist at higher energy levels. When electrons return to a lower energy level, they emit energy in the form of light known as photons.

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14
Q

Light is ___ as electron falls back to a lower energy level

A

emitted

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15
Q

Electron ___ energy and is excited to unstable energy level.

A

absorbs

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16
Q

What do electrons exist as?

A

both particles and waves (like photons)

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17
Q

What are orbitals described by?

A

4 quantum numbers

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18
Q

How many electrons can an orbital have?

A

2

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19
Q

Can there be multiple orbitals?

A

yes

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20
Q

what letter represents the principal quantum number?

A

n

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21
Q

What is the range for n?

A

1,2,3…

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22
Q

What does the principal quantum number represent?

A

the electron shell (distance form the nucleus)

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23
Q

What letter represents the angular quantum number?

A

l

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24
Q

What is the range for l?

A

l=0,….(n-1)

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25
Q

What letter represents the magnetic quantum number ?

A

m1

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26
Q

What is the range for m1?

A

m1= -l,…,0,…,l

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27
Q

What does the angular quantum number (l) govern?

A

the subshells

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28
Q

What are the letters used for the subshells?

A

s,p,d,f

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29
Q

when l=0, what can ml only be?

A

0

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30
Q

What is the quantum number for electron spin?

A

ms (+1/2 & -1/2)

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31
Q

What happens when electrons of the same charge are spinning in opposite directions?

A

they won’t repel each other’s negative charge

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32
Q

What shape does the s orbital have?

A

a spherical shape

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33
Q

what does l equal in the s orbital?

A

0

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34
Q

what shape do the p orbitals have?

A

p orbitals have a dumbell/egg shape

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35
Q

What are the values for ml in the p orbital?

A

ml= -1,0,1

36
Q

What does l equal in the p orbital?

A

1

37
Q

What shape does the d orbital have?

A

a clover shape

38
Q

What are the values for ml in the d orbital?

A

ml= 1, 0, 2, -1, -2

39
Q

What does l equal in the d orbital?

A

2

40
Q

What shape does the f orbital have?

A

there is no distinct shape

41
Q

What are the value for ml in the f orbital?

A

ml= -3, -2, -1, 0, 1, 2, 3,

42
Q

what does l equal in the f orbital?

A

3

43
Q

What elements are alkaline metals?

A

Group 1: Hydrogen (H), Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Caesium (Cs), Francium (Fr)

44
Q

What elements are Alkaline earth metals?

A

Group 2: Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba), Radium (Ra)

45
Q

what elements are Halogens?

A

Group 7: Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I), Astatine (As)

46
Q

What elements are Noble Gases?

A

Group 8: Helium (He), Neon (Ne)m Argon (Ar), Krypton (Kr), Xenon (Xe), Radon (Rn)

47
Q

Are Groups on the periodic table left to right, or up and down?

A

Up and Down

48
Q

Are Periods on the periodic table left to right or up and down?

A

Left to right

49
Q

What is the reactivity trend on the periodic table?

A

Reactivity increases as you go down the column

50
Q

Groups on the periodic table have similar chemical properties true or false?

A

True

51
Q

Where do electrons exist?

A

in orbitals

52
Q

What are the two rules to the Pauli Exclusion Principle?

A
  1. No two electrons in an atom may have the same set of four quantum numbers
  2. No orbital may have more than two electrons and they must have opposite spins
53
Q

Aufbau’s Principle rule 2

A

Orbitals are filled in order of incresing energy

54
Q

Where will electrons always go?

A

to the lowest energy state

55
Q

When is Aufbaus’s principle violated?

A

If the electron is given energy; because this will cause the electron to jump to a higher energy state

56
Q

Write out the electron configuration for Ga

A

1s^2, 2s^2, 3s^2, 3p^6, 4s^2, 3d^10,4p^1

57
Q

Hund’s Rule

A

For electrons with degenerate orbitals, the lowest energy is attained when the number of electrons having the same spin is maximized

58
Q

What do we use to do a condensed electron configuration?

A

The noble gas in the period above

59
Q

What is Zeff?

A

Z effective is how much positive charge an electron “sees” based on number of electrons between

60
Q

How do you calculate the effective nuclear charge

A

Zeff= (number of protons [atomic #]- (the number of core electrons [row it’s in])

61
Q

Example: What is the effective nuclear charge for an electron in the n=2 in an atom of fluorine?

A

Zeff=9-2
Answer = 7

62
Q

What are core electrons?

A

are all electrons in inner energy levels including completely filled d and f subshells

63
Q

What is electron shielding?

A

the blocking of valance shell electrons attraction by the nucleus, due to the presence of inner-shell electrons (think of in-class college bar analogy)

64
Q

Where does the Zeff trend increase?

A

As you move to the right on the periodic table

65
Q

How is the size of an atom measured?

A

atomic radius

66
Q

What is the atomic radius trend?

A

atomic radius increases as you move down & to the left of the periodic table

67
Q

What is the largest element?

A

Francium

68
Q

Cations

A

loses electrons, has a positive charge, shrinks because it’s losing electrons

69
Q

Anions

A

gains electrons, negative charge, grows because it’s gaining electrons, larger than their parent atom

70
Q

True or False: Cations are larger than their parent atom

A

False, cations are smaller due to losing electrons

71
Q

True or False: Anions are larger than their parent atom

A

True

72
Q

Arrange Mg^2+, Ca^2+, Ca in order of decreasing radius (largest to smallest)

A

Ca, Ca^2+, Mg^2+

73
Q

What is the ionic radius trend?

A

As you move down a column on the periodic table the ionic radius increases

74
Q

What is an isoelectronic series?

A

a group of atoms/ions that have the same number of electrons

75
Q

What will transition metal cations do?

A

they will remove electrons from the s subshell before the d subshell because they have a partially filled d block

76
Q

What is ionization energy?

A

It is the amount of energy required to remove an electron from an atom/ion in a gaseous state (energy needed to make a cation)

77
Q

What is the increasing first ionization energy trend?

A

Up and to the right

78
Q

What element has the highest first ionization energy?

A

helium

79
Q

What is electron affinity?

A

The energy released when an electron is added to the gaseous state of an atom/ion (makes an anion)

80
Q

What are most electron affinities?

A

negative (releasing)

81
Q

What are all ionization energies?

A

positive (absorbing)

82
Q

What is metallic character?

A

It is the measure of the degree to which an element exhibits the chemical and physical properties of a metal

83
Q

what are some metallic characteristics?

A

lustrous, high melting point, and very conductive

84
Q

What is the metallic trend?

A

Increases down and to the left

85
Q

What element is the most metallic?

A

Francium

Chemistry 1 (4 decks)

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