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General Chemistry > TEST 3 > Flashcards

TEST 3 Flashcards

(54 cards)

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1
Q

What are the four periodic trends?

A

Atomic radius, Ionization energy, Electron affinity, Electronegativity

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2
Q

Difference between covalent and metallic radii

A

Covalent radius is half the distance between two covalently bonded atoms - Metallic radius is half thee distance between tow metal atoms in a solid crystal

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3
Q

What in the trend in radius across the PT

A

Decreases across each period, Increases down a group

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4
Q

What is atomic radius dependent on?

A

the effective charge of an atom, Z_eff

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5
Q

What is Z_eff?

A

It is the effective charge of an atom, the charge minus the shielding of the lower shells

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6
Q

Why does radius decrease across a period?

A

The atom’s effective charges grows, pulling the valence electrons closer to the nucleus

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7
Q

Relationship between shells, subshells and shielding

A

Shielding is generally larger between shells and smaller between subshells

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8
Q

What is the relationship between protons, electrons and atomic radius?

A

More protons than electrons means smaller radius (greater attraction)
More electrons than protons means larger radius (weaker attraction)

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9
Q

What is an isoelectronic series?

A

Variation in protons of an atom

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10
Q

What is ionization energy?

A

The energy required to pull an electron off of a gaseous atom

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11
Q

Why does ionization energy increase as more electrons are removed?

A

Less electrons, greater proton ration, greater effective charge, greater attraction

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12
Q

Why does ionization energy jump when there is a change of shell?

A

Full shells are more stable and are harder to break apart

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13
Q

What is the trend in first ionization energy across the PT?

A

Increases across a period and decreases down a group (proportional to effective charge)

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14
Q

What is electron affinity?

A

Change in energy caused by the addition of an electron to a gaseous atom to form an anion

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15
Q

What is the relationship between stability and EA

A

The more negative the EA, the more stable an anion is

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16
Q

Relationship between EA and Z_eff

A

EA becomes more negative as effective charge increases

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17
Q

What is the trend in EA across the PT?

A

Becomes more negative going across a period, becomes more positive going down a group

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18
Q

Which group has the highest EA and why?

A

Group 7A since only 1 electron is needed to form an octet

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19
Q

Which groups have the lowest EA and why?

A

Group 2A and 8A since they already have their highest shells filled

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20
Q

What three forces exist between two bonded atoms?

A

Electron-electron repulsion, Proton-proton repulsion, Proton-Electron attraction

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21
Q

What in the BOND LENGTH in terms of bond forces?

A

The bond length is the point where bond forces cancel out

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22
Q

What is bond polarity? How can it be determined?

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A

The ability of an atom in a bond to attract shared electrons. Found with electronegativity

23
Q

What is the trend for electronegativity across the PT?

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A

Across a period and up a group, EN increases
(F highest, Fr lowest)

24
Q

What is a polar bond referred to as?

25
What is bond dipole moment and what is its unit?
The product between the distance and charge of the bonds, measured is debyes [D]
26
Relationship between polarity and dipole moment
Larger dipole moment means greater polarity
27
Relationship between distance in PT and ΔEN
Larger distance in PT generally means greater ΔEN
28
Polarity ranking of bonds
Ionic, polar covalent, covalent
29
What are the three bond types?
Ionic, covalent, polar covalent
30
What are bond energies (BE or BDE)
The energy required to break a bond
31
Formation/breaking exothermic or endothermic
Breaking: endothermic, forming: exothermic
32
How to find enthalpy of a reaction
The difference between the energy of the bonds made and the energy of the bonds broken
33
Difference between bonding pairs and lone pairs
Bonding pairs are electrons shared between two atoms Lone pairs are electrons left over on atoms
34
What are the three functions of the Localized Electron Bonding model
1) Description and arrangement of valence electrons 2) Prediction of molecular geometry 3) Description of orbitals // Hybridization
35
What are the exceptions to the octet rule
H is filled with 2 e- Be is filled with 4 e- B is filled with 6 e- Most elements in period 3 and above can have more than 8 e-
36
Steps to build LS (1-3)
1: Find total Ve 2: determine central atom, placing outer atoms around 3: Add electrons until all surrounding atoms are filled
37
Which outer atoms should be filled first for LS?
Atoms with greater electronegativity
38
Steps to build LS (4-6)
4: Add remaining e- onto central atom 5: Predict geometry, indicate angles 6: If octet rule is not satisfied for required atoms, use multi bonds to fill in extra electrons
39
Steps to build LS (7-9)
7: Indicate charge of a molecule using square brackets 8: Show resonance structures 9: Show resonance hybrid
40
What are resonance structures?
The different possible configurations of a molecules using multi-bonds
41
What makes RS equivalent and non-equivalent? Lewis structures?
Same # of bonds and same surrounding atoms vs different number of bonds (same applies to LS)
41
What is a resonance structure?
The true structure of a molecules based on the greatest stability
41
What is formal charge? How to find it?
The relationship between the valence electrons of an atom before and after bonding Group number (or VE) - (1/2 #BP + #LP)
42
General states of different atoms in molecules
C: 4 BP H: 1 BP O: 2 BP 2 LP N: 3 BP 1 LP S: 2 BP 2 LP Halogens: 1 BP 3 LP
43
How are hybridized orbitals formed?
mixing of valence orbitals with lower orbitals (ex: SP3)
44
What are valence orbitals and which orbitals can hybridize?
Valence orbitals are the orbitals in the highest shell of the electron config. ONLY VO and VE hybridize.
45
Two bond variations and what they mean
Sigma bonds: Single bonds and first bond of multi bonds Pi bonds: Second and third bonds of multi bonds
46
What angle do triple bonds have?
Always 180
47
Which pair(s) are counted in hybridization?
BOTH LP and BP
48
How are LP placed when there are 5 bonds total?
Equatorial positions
49
How are LP placed when there are 6 bonds total?
Axial positions
50
Example of an isoelectric series
Al 3+ , Mg 2+ , Na + , F - (all 10 e-, different # protons)
51
How are different planes represented when drawing molecular structures?
Hatched wedge: Back Triangle: Front Line: On axis
52
Order of bond lengths
Single > Double > Triple

General Chemistry (5 decks)

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