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flashcards! > AP Chem. Ch.8-9 > Flashcards

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
Q

How to find formal change

A
  • 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
Q

Which are the 3 types of ions that dont follow the octet rule?

A
  • ions or molecules with an odd number of electrons
  • ions or molecules with less than an octet
  • ions or molecules
26
Q

How many bonds does H need to b stable?

A

1 bond( 2 electrons)

27
Q

How many bonds does Be need for it to b stable??

A

2 bonds( 4 electrons)

28
Q

How many bonds does B need for it to be stable??

A

3 bonds( 6 electrons)

29
Q

Atoms from the ____ period(and below) can accomodate more than an octet.

A

Third. _ _

Ex: PCl5, SF4, AsF6 , and ICl4

30
Q

The strength of a bond is measured by determining how much energy is required to break the bond.

A

Bond enthalpy

31
Q

Why are the average bond enthalpies of covalent bonds positive??

A

B/c bond breaking is an endothermic process

32
Q

Bond forming should be _____

A

Exothermic

33
Q

As number of bonds increases…

A

The bond length decreases

The bond enthalpy increases

34
Q

What factor plays an important role in the molecule reactivity?

A

The shape of a molecule

35
Q

What is the shape of a molecule determined by??

A

By its bond angles

36
Q

What does VSEPR theory stand for?

A 
Valence
Shell
Electron
Pair 
Repulsion
37
Q

“The best arrangement of a given number of electron is the one that __________ repulsions among them”

A

Minimizes

38
Q

Electron pairs, bonding and nonbonding, _____ each other.

A

Repel

39
Q

Electrons pairs can be referred as

A

Electron domains

40
Q

Predicted bond angle for 2 electron domains.(linear)

A

180

41
Q

Predicted bond length for 3 electron domain.( trigonal planar)

A

120

42
Q

Predicted bond length for 4 electron domains.( tetrahedral)

A

109.5

43
Q

Predicted bond length for 5 electron domains. ( trigonal bypiramidal)

A

120, 90

44
Q

Predicted bond length for 6 electron domains.( octahedral)

A

90

45
Q

Molecular geometries that are possible for Trigonal planar:

A
  • trigonal planar

- bent

46
Q

Molecular geometries that are possible for Tetrahedral:

A
  • tetrahedral
  • Trigonal pyramidal
  • bent
47
Q

Molecular geometries that are possible for Trigonal bypiramidal.

A
  • trigonal pyramidal
  • seesaw
  • T-shaped
  • linear
48
Q

Molecular geometries that are possible for Octahedral:

A
  • octahedral
  • square pyramidal
  • square planar
49
Q

what does the Heisenberg uncertainty principle state?

A

The position and the momentum of an electron can never be simultaneously, exactly known.

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