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Chemistry > Exam 2 > Flashcards

Exam 2 Flashcards

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1
Q

All s orbitals are spheres so..

A

They have no angular dependence on orientation

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2
Q

When does the orbital size increase?

A

With and increase in the value of quantum number N

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3
Q

All orbitals with an N>= 2 have…?

A

A subs hell containing 3 P orbitals

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4
Q

What is a node?

A

A plane in which the probability of finding an electron is 0 (zero electron density)

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5
Q

How many nodes does each orbital, s, p and d have?

A

1S=0 because 2s and 3s have radial nodes
P=1
D=2

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6
Q

For the same N value what is the relationship between P and S orbitals and PE?

A

With the same number N a P orbital will have higher PE because the electron density is farther from the nucleus

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7
Q

What is an orbital?

A

The electron occupies a 3 dimensional space called an orbital

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8
Q

What does an orbital show about the electron?

A

The volume of where the electron is 90% of the time

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9
Q

Tell me about the density of the 1s orbital

A

It’s greatest at its nucleus

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10
Q

What is the Aufbau Principal?

A

Electrons are placed in the lowest energy orbitals and each orbital can only obtain 2 electrons that are spin paired (opp)

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11
Q

What is the trend for probability density?

A

Highest at the Nucleus and lowest away

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12
Q

In general what is a shell?

A

Refers to an energy level

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13
Q

When are electrons in the same shell?

A

Electrons are in the same shell if they have the same N value and same type of orbital (s,p,d,f)
Each orbital has different energy

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14
Q

As N increases what does E do?

A

Increase

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15
Q

What type of cations do S block elements form?

A

Monoatomic cations by losing all their outer shell electrons leaving it with the electron configuration of the Noble Gas directly preceding it

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16
Q

What kind of anion does a P block element form?

A

A monoatomic anion by gaining enough electrons to fill its valence shell and has the configuration of the noble gas at the end of its row

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17
Q

What is an isoelectric ion?

A

Ions with the same electron configuration, (Na+,F-,Ne)

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18
Q

What do electrons in orbitals with the highest N values do?

A

They ionize first and are farther from the nucleus. So as N increases, D increases and thus E increases

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19
Q

What happens to the size of an atom as atomic number increases and you’re going down a group of elements?

A

Atom size increases

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20
Q

What happens to atom size with an increase in atomic number but going left to right on the table?

A

Size decreases

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21
Q

Where are the valence electrons?

A

In the highest energy level ( whatever # is the highest and the orbital containing it)
ANYTHING AFTER THE NOBLE GAS CONFIGURATION

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22
Q

Any element with an electron configuration with that of a noble gas is…?

A

The most abundant and thus stable

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23
Q

Generally what is the PE of electrons?

A

Basically 0 because they are infinitely far away from the nucleus

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24
Q

What is ionization energy?

A

The energy required (KJ / mil) to remove 1 mile of electrons from 1 mile of gas-phase atoms or ions in their ground state
ALWAYS REQUIRES ENERGY TO REMOVE ELECTRONS

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25
Q

How to find the total I.E.

A

It’s the sum of the ionization energies

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26
Q

Which orbital takes more energy to remove an electron? P or S?

A

S

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27
Q

What does the repulsion of electrons in electron configurations do?

A

They have higher energy and thus require less energy to be ionized

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28
Q

Periodic trend of I.E.?

A

I.E. Decreases from top to bottom of every group on the periodic table

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29
Q

Which orbital: Density decreases as distance increases

A

S orbital

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30
Q

If you have an anion which way on P table do you go?

A

⬆️

31
Q

If you have a cation which way on the P table do you go?

A

⬇️

32
Q

Why are spheres good shields?

A

Because they don’t have nodes

33
Q

Which electrons shield the best?

A

Core electrons, so maximal shielding when an electron is added to a completely full shell, then shielding diminishes from there

34
Q

What does adding or subtracting electrons on a regular ion do?

A

Dramatically change the size

35
Q

As atomic radius (and thus atom size) decrease what happens to I.E.?

A

Increases

36
Q

What is the order of screening effectiveness?

A

S>P>D>F

37
Q

Which is better at screening- electrons in inner shells or the same shell?

A

Inner shells

38
Q

Which elements have the highest and lowest Zeff?

A

He is the highest

Cs is the lowest

39
Q

Which is larger- anions or a neutral atom of the same element?

A

Anions

40
Q

Which is bigger- cations or a neutral atom of the same element?

A

Neutral atom of the same element

41
Q

What is valence?

A

The capacity of the atoms of an element to form chemical bonds

42
Q

What is electrostatic potetinal?

A

The energy a charged particle has because of its position relative to another charged particle

43
Q

How is electrostatic potential related to the product of the charges of the particles and the distance between them?

A

Directly

Inversely

44
Q

What is the constant in the electrostatic potential energy equation?

A

2.31X10^-19 J•nm

45
Q

What energy is repulsion accompanied by?

A

Positive

46
Q

What energy is attraction associated with?

A

Negative- the greater the attraction the more negative the electrostatic PE

47
Q

What is lattice energy?

A

The stability afforded by packing ions together

Energy is released when a crystal lattice of ions is formed from the ions

48
Q

What is bond length?

A

The distance between the nuclear centers of two atoms joined together in a bond
•have values close to the sum of the atomic radius of the atoms involved

49
Q

What is bond energy? Aka bond strength

A

The energy needed to break 1 mole of a covalent bond in a molecule or polyatomic ion in the gas phase

50
Q

What is a metallic bond?

A

Consists of the nuclei of metal atoms surrounded by a “sea” of shared electrons

51
Q

What is electron mobility?

A

Metals are good conductors of electricy

52
Q

What is the photoelectric effect?

A

States that photons must have a frequency greater than or equal to a frequency that is characteristic of a solid

53
Q

What is the relationship between work function, energy, and ionization energy?

A

Smallest work function, smallest r energy and thus lowest ionization energy

54
Q

What happens if the photon doesn’t exactly match a minimum frequency?

A

It won’t do anything, but in the photoelectric effect the excess energy is converted to KE

55
Q

As Q1 • Q2 increases…

A

Potential energy becomes more negative

56
Q

As D decreases what happens to PE?

A

It becomes more negative (stable)

57
Q

When do ionic bonds generally form?

A

When atoms of low I.E. (Which is not difficult to lose an e-) and atoms with high negative electron affinities (which is favorable to gain an e-) get together

58
Q

What are oxyanions

A

An anion containing one or more oxygen atoms bonded to another element

59
Q

When do you add ate to the end of an oxyanion?

A

When it has the larger number of oxygen atoms

60
Q

When do you add ite to the end of an oxyanion?

A

When it has less oxygen atoms

61
Q

What is a binary molecular compound?

A

A compound that combines two nonmetallic elements

62
Q

What is a binary acid?

A

The most simple acid, hydrogen is bonded to another nonmetallic element

63
Q

What does adding an electron do to an atom?

A

Reduces the potential energy

64
Q

What happens when you bring like charges together?

A

The PE sky rockets

65
Q

What happens when the PE is the lowest?

A

It is the most stable

It’s also where bond length is measured

66
Q

Does it require energy or is energy released when breaking a lattice sort?

A

Work and energy is used

67
Q

Does energy increase or decrease when bringing ions together to make a lattice?

A

Decrease energy

68
Q

Do covalent bonds have electrostatic force?

A

No because ions aren’t involved

69
Q

Which type of bond is more stable, covalent or ionic?

A

Covalent

70
Q

Why is a molecular orbital more stable?

A

Because the electron is near 2 nucleus

71
Q

How to name ionic compounds?

A

List the name of the cation then prefix of the anion followed by “ide”

72
Q

What do you do to name ionic compounds of transition metal cations?

A

CrCl2 - chromium (2) chloride so chromous chloride OUS for smaller #
CrCl3- chromium (3) chloride so chromic chloride IC is for the smaller number

73
Q

What is a polar covalent bond?

A

A bond resulting from unequal sharing of bonding pairs of electrons between atoms-HCl

74
Q

What is a dipole?

A

Means there is a slightly positive and a slightly negative pole on the atom (like a battery)

Chemistry (2 decks)

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