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CHEM > Exam 1 > Flashcards

Exam 1 Flashcards

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1
Q

The law of conservation of matter/the law of conservation of mass–energy

A

Initial mass and energy=Final mass and energy

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2
Q

The law of conservation of matter is also known as the law of conservation of mass–energy. Initially proposed by Albert Einstein, this law suggests that while the total mass and energy of a system is conserved, mass and energy can interconvert. We’ll discuss energy in much greater detail in Chapter 11: Chemical Kinetics.

A
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3
Q

White light is a mixture of _____________________

A

All visible light colors

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4
Q

What is color determined by?

A

The only wavelength of light that isn’t absorbed (The reflected color is the one we see)

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5
Q

What is frequency? What are the unit and symbols?

A

The number of waves passing a given point per unit of time?

Hertz, v

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6
Q

Frequency (v) and wavelength (λ) are ___________ proportional

A

inversely

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7
Q

What is the energy of a wave proportional to?

A

Amplitude and frequency of a wave

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8
Q

What speed do all electromagnetic waves move at?

A

Light speed, c, 3x10^8 m/s

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9
Q

What happens when traveling waves encounter an opening in a barrier?

A

They bend around it, and it looks like the wave is starting from the opening

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10
Q

How do the waves meet when they encounter an opening in a barrier?

A

Interact with alternating constructive and destructive waves

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11
Q

What does the EM spectrum include?

A

All wavelengths of EM radiation

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12
Q

What are the types of EM radiation with increasing frequency?

A

GXUVIMR

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13
Q

Johannes Rydberg

A

Analyzed the spectrum of Hydrogen, created Rydberg equation
1/λ=Rh(1/nf^2-1/ni^2)

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14
Q

Max Planck

A

Discovered energy emitted in packets called quanta and proposed that atoms needed to move at a minimum speed to emit energy

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15
Q

Albert Einstein

A

Expanded on Planck’s work, interpreted Hertz’ PE effect. Proposed the existence of photons, small particles of EM radiation.

Applied Planck’s formulas to photons

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16
Q

Heinrich Hertz

A

Observed that when a metal absorbs sufficient energy its electrons are ejected from the surface. Known as “photoelectric effect”. Requires a certain frequency

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17
Q

Neils Bohr

A

Merged Rutherford’s nuclear model of the atom with Planck’s and Einstein’s ideas about quantum theory to create the Bohr model

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18
Q

Louis de Broglie

A

Said all subatomic matter in motion could be treated as a wave

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19
Q

Heisenberg

A

Can’t know location and momentum of an e- with absolute certainty

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20
Q

When an element absorbs energy, a unique ________ of light is emitted

A

absorbs

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21
Q

When emitted light is directed into a prism, a

A
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22
Q

What is blackbody radiation?

A
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23
Q

What is the emission of BB radiation called?

A

Incandescence

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24
Q

What is Planck’s formula?

A

E=hv=hλ

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25
Q

What is the photoelectric effect?

A

When the intensity of light is above v=o, # e- increases with intensity and KE of e- increases with frequency

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26
Q

How do you calculate the minimum energy needed to remove an electron?

A

The threshold frequency-
E0=hv0

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27
Q

Photoelectric effect: When v>v0, the excess energy needed to remove an e- is given as

A

Kinetic energy

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28
Q

How can you calculate wavelength using energy and planck’s constant?

A

E=λh

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29
Q

How can you calculate the number of photons in a beam?

A

E pulse (J)/E photon (j)=# of photons

30
Q

How do you calculate the energy of a photon?

A

E=hv=hc/λ

31
Q

What are the main ideas of the Bohr model?

A

Electrons can only move in fixed orbits around the nucleus which are described using positive integers

32
Q

When n=1, this is called the

A

Bohr radius

33
Q

What is the closest an electron can be to the nucleus? (Why e- don’t crash into the nucleus)

A

n=1

34
Q

What did Bohr propose about each orbit? What was the formula?

A

It had an assigned energy to it- En=-2.18 x 10^-18J (1/n^2)

35
Q

What is Coulomb’s law? (not the formula)

A

The coulombic potential energy is dependent on the charges of the particles and the distance between them

36
Q

What is the formula for Coulomb’s law?

A

E= kQ1Q2/d
k=8.99x10^9nxm^2/c^2

37
Q

Why is Bohr’s equation negative

A

To reflect difference in charges between e- and p+

38
Q

When do you use Delta e=-2.18 x 10^-18J (1/nf^2-1/ni^2)

A

Photoemission questions

39
Q

Hund’s Rule

A

Electrons won’t enter an orbital with an electron if there’s one that is empty already

40
Q

Aufbau Principle

A

Lower orbitals are filled before higher ones

41
Q

Pauli-exclusion principle

A

Electrons will never have the same set of 4 quantum numbers

42
Q

What is unique about transition metal’s configuration? HOWEVER, if you are being asked about a transition metal, after you find the Aufbau (lowest energy answer), look again.

A

S electrons move to the D spaces a lot to create symmetry

43
Q

What is the l value for s?

A

0

44
Q

What is the l value for p?

A

1

45
Q

What is the l value for d?

A

2

46
Q

What is the l value for f?

A

3

47
Q

What do all alkali metals have in their subshells? [noble gas]s1 (aka half filled s subshells) and the alkaline earth metals are all [noble gas]s2 (aka filled s subshells) in terms of their valence (outermost shell) configuration

A

Half filled subshells

48
Q

What do all alkaline earth metals have in their subshells?

A

Filled subshells

49
Q

When do transition metals need to move over one electron?

A
50
Q

What groups does the p subshell apply to?

A

Last 6 groups on the PT

51
Q

How many degenerate orbitals does the p subshell have? What are they? How many electrons can it hold?

A

3, (-1, 0, 1), 6

52
Q

What do all noble gases have in terms of their shells?

A

Completely filled subshells (Filled s and filled p and f except for helium)

53
Q

The group that starts with nitrogen contains all of the elements that are [noble gas]s2p3 which are half-filled (aka have one electron in each of the three degenerate orbitals) in terms of their valence configuration. As such, this column of elements is relatively stable.

A
54
Q

What groups do the d subshells correspond to?

A

The middle 10 groups on the PT

55
Q

What is the ml for d?

A

-2, -1, 0, 1, 2

56
Q

How many electrons can the d subshell hold?

A

10

57
Q

The group that starts with manganese contains all of the elements that are [noble gas]s2d5 which are half-filled (aka have one electron in each of the five degenerate orbitals) in terms of their valence configuration. As such, this column of elements is relatively stable.

A
58
Q

The group that starts with zinc contains all the elements are [noble gas]s2d10 which are filled (aka have two electrons in each of the five degenerate orbitals) in terms of their valence configuration. As such, this column of elements is even more stable.

A
59
Q

The experiment that determined that electrons were negatively charged particles was

A

The Thomson cathode ray experiment

60
Q

_________ bonds share e-

A

Covalent

61
Q

__________ bonds have an attraction between 2 particles

A

Ionic

62
Q

Ionic compounds arrange themselves in an array of ________, while molecular compounds only form a few discrete _______

A

ions, bonds

63
Q

Who proposed e- in H atoms can only have certain energies?

A

Bohr

64
Q

What is the value of L for the orbital shown below?

A
65
Q

Provide the quantum numbers and related information for the following orbital, 4f.

What is the principal quantum number, n?

A

4

66
Q

Provide the quantum numbers and related information for the following orbital, 4f.

What is the angular momentum quantum number, l?

A

3

67
Q

Provide the quantum numbers and related information for the following orbital, 4f.

What is the number of degenerate orbitals based on the magnetic quantum number?

A

7

68
Q

What is the formula for ml?

A

2l+1

69
Q

What is the formula for finding radial nodes?

A

n-l-1

70
Q

How many orbitals are present in the g shell?

A

9

71
Q
A

CHEM (10 decks)

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