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Chemistry 10 Honors > Chemical Bonds I > Flashcards

Chemical Bonds I Flashcards

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1
Q

Chemical Bonds

A
  1. Attraction between atoms or ions

2. Are due to the attraction between the positive nucleus and the negative electrons

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2
Q

Potential Energy

A

Stored in bonds between atoms/ions

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3
Q

Chemical Energy

A

Energy involved in making/breaking bonds

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4
Q

Energy Changes in Bonds

A
  1. When two atoms are bonded –> lower/stable potential energy level
  2. When stronger bonds form –> Exothermic Reaction + Less potential energy
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5
Q

Relationship between stabiltilty and potential energy

A

Inverse

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6
Q

Exothermic vs Endothermic

A

Exothermic: Stability is high, potential energy is low when compared to reactants
Endothermic: Stability is low, potential energy is high when compared to reactants

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7
Q

Endothermic/Exothermic Diagram

A

Bottom is potential energy

Top is kinetic energy

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8
Q

Electronegativity

A

0-.3 –> NPC
.3-1.7 exclusive –> PC
>1.7 inclusive –> I

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9
Q

Ionic Bonds

A

Attraction between ions

Nonmetal and Metal

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10
Q

Lewis Structures for Ionic Bonds

A

Must have charges

May draw arrows, or have nonmetal have a full shell

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11
Q

Properties of Ionic Compounds

A 
As solids don't conduct electricity
When melted/in aqueous solution conduct electricity
High melting points
Have crystalline lattice structure
Very strong
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12
Q

Covalant Bonds

A

Either equally/unequally shared electrons

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13
Q

NPC

A

Shared equally between two nonmetals

END is

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14
Q

PC

A

Shared unequally between two nonmetallic atoms

.3

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15
Q

Properties of Covalant Compounds

A

Low melting Point
Dull
Brittle
Nonconductive

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16
Q

Network Solid

A

Chemical compound where the atoms are bonded covalently in a continuous network
Entire network is considered a molecule

17
Q

Properties of Network Solids

A

Very high melting point
Very strong covalent bonds
Very hard
Not soluble in water

18
Q

Examples of Network Solids

A

Diamond –> C
Silicon Dioxide –> Si02
Graphite –> C in two dimensional layers

19
Q

Coordinate Covalent Bonds

A

When both electrons from a bond are shared by only one of the two atoms

20
Q

Metallic Bonds

A

Electrons in solid metals are free travel atom to atom
Metals became cations due to loss of electrons
Attraction between the mobile electrons and the metals cause a strong bond to form
Called Sea of Electrons

21
Q

Properties of Metallic bonds

A

Luster
Ductile
Malleable
Conductor

22
Q

Localized Electron Model

A

Electron Pairs are assumed to be localized on a particular atom or in the space between two atoms.
Description of valence electron arrangement (Lewis Structure)
VSEPR
Description of atomic orbital types used to share electrons or hold lone pairs

23
Q

Lone Pair Electrons

A

Electrons located on an atom

24
Q

Bonding Electrons

A

Electrons found in the space between the atoms

25
Q

2nd Row Elements

A

C,N,O,F use octet rule

Often have fewer than eight electrons, they are very reactive

26
Q

3rd Row and heavier elements

A

Can exceed the octet rule, using empty d valence orbitals

27
Q

VSEPR

A

Valence Shell Electron Pair Repulsion

28
Q

Intramolecular

A

Involved in bringing atoms together to a compound
Ionic
Polar Covalent
Nonpolar Covalent

29
Q

Intermolecular

A

Involved in bringing molecules together
Dipole-Dipole - Strong, Unequal/Partial charges
Hydrogen Bonds (H to F,O,N) - Strongest
Weak/Van Dar Waal’s - Weakest

30
Q

Weak Intermolecular Forces

A

Small nonpolar molecules, best in liquid/solid phases with low temp and high pressure
Stronger when closer together
Smaller the molecule –> weak
Larger the molecule –> strong
Smaller nonpolar molecules, tend to be gases at room temperature, give them low boiling points –> Noble Gasses
Larger nonpolar molecules, tend to be liquids and solids at room temperature
Diatomic Molecules are also examples

Chemistry 10 Honors (4 decks)

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