AP Chem. Ch.8-9 Flashcards

0
Q

Driving force among all types of bonding?

A

Electrostatic

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1
Q

Which are the three basic types of bonds?

A

Ionic
Covalent
Metallic

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2
Q
  • electrostatic attractions between ions

- metal w/ nonmetal

A

Ionic bond

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3
Q
  • sharing of electrons

- nonmetal w/ nonmetal

A

Covalent bond

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4
Q

-metal atoms bonded to several other atoms

Metal w/ metal

A

Metallic

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5
Q

All chemical bonds form b/c the electron-proton attraction _______ the potential energy of the system as the bond forms

A

Lowers

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6
Q

Balance between the attractiobs of the oppositely charged particles and repulsions of the like charged particles

A

Distance between the bonded particles

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7
Q

Electrons involved in bonding

A

Balance electrons

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8
Q

Where are balance electrons found?

A

In the incomplete, outer most shell of an atom.

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9
Q

Atoms tend to gain, lose, or share electrons until they are surrounded by eight valence electrons

A

Octet rule

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10
Q

Which subshells does an octet consist of?

A

S^2, P^6 subshells

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11
Q
  • Energy required to completely separate a mole of a solid ionic compound into its gaseous ions.
  • increases with the CHARGE on the ions.
  • increases w/ the DECREASING SIZE of ions.
A

Lattice energy

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12
Q

What 2 factors affect lattice energy??

A

Charge and size

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13
Q

Thermodynamic cycle that analyzes lattice energy precisely.

A

Born-harber cycle

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14
Q

Three electrostatic interactions in covalent bonds:

A
  • Attraction between electrons and nuclei
  • repulsions between electrons
  • repulsions between nuclei
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15
Q

Sharing of 1 pair of e- bettwen atoms.

A

Single covalent bond

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16
Q

Pair of electrons that is not being shared.

A

Unshared pair

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17
Q

Which atoms can form multiple bonds??

A

C, N, O, S

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18
Q

Sharing of 2 pairs of e- between atoms.

A

Double covalent bond

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19
Q

Aharing of 3 pairs of electrons between atoms.

A

Triple covalent bond

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20
Q

Equal sharing of electrons.

A

Nonpolar covalent

21
Q

Unequal sharing of electrons

A

Polar covalent

22
Q

The ability of atoms in a molecule to attract electrons to themselves
Increases accros the period, decreases down a column

A

Electronegativity

23
Q

Representations of molecules shoeing all electrons, bonding and nonbonding

A

Lewis structures

24
How to find formal change
- count # of valence electrons - add up the number of unshared electrons to half the number of shared electrons. - subtract this value from the # of valence electrons.
25
Which are the 3 types of ions that dont follow the octet rule?
- ions or molecules with an odd number of electrons - ions or molecules with less than an octet - ions or molecules
26
How many bonds does H need to b stable?
1 bond( 2 electrons)
27
How many bonds does Be need for it to b stable??
2 bonds( 4 electrons)
28
How many bonds does B need for it to be stable??
3 bonds( 6 electrons)
29
Atoms from the ____ period(and below) can accomodate more than an octet.
Third. _ _ | Ex: PCl5, SF4, AsF6 , and ICl4
30
The strength of a bond is measured by determining how much energy is required to break the bond.
Bond enthalpy
31
Why are the average bond enthalpies of covalent bonds positive??
B/c bond breaking is an endothermic process
32
Bond forming should be _____
Exothermic
33
As number of bonds increases...
The bond length decreases | The bond enthalpy increases
34
What factor plays an important role in the molecule reactivity?
The shape of a molecule
35
What is the shape of a molecule determined by??
By its bond angles
36
What does VSEPR theory stand for?
``` Valence Shell Electron Pair Repulsion ```
37
"The best arrangement of a given number of electron is the one that __________ repulsions among them"
Minimizes
38
Electron pairs, bonding and nonbonding, _____ each other.
Repel
39
Electrons pairs can be referred as
Electron domains
40
Predicted bond angle for 2 electron domains.(linear)
180
41
Predicted bond length for 3 electron domain.( trigonal planar)
120
42
Predicted bond length for 4 electron domains.( tetrahedral)
109.5
43
Predicted bond length for 5 electron domains. ( trigonal bypiramidal)
120, 90
44
Predicted bond length for 6 electron domains.( octahedral)
90
45
Molecular geometries that are possible for Trigonal planar:
- trigonal planar | - bent
46
Molecular geometries that are possible for Tetrahedral:
- tetrahedral - Trigonal pyramidal - bent
47
Molecular geometries that are possible for Trigonal bypiramidal.
- trigonal pyramidal - seesaw - T-shaped - linear
48
Molecular geometries that are possible for Octahedral:
- octahedral - square pyramidal - square planar
49
what does the Heisenberg uncertainty principle state?
The position and the momentum of an electron can never be simultaneously, exactly known.