Covalent Bonding Flashcards

1
Q

Covalent bond:

A

a chemical bond formed by the sharing of e- btwn two atoms (non and non)

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2
Q

molecule:

A

a neutral group of atoms that are held together by covalent bonds

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3
Q

molecular compound:

A

a chemical compound whose simplest units are molecules

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4
Q

chemical formula:

A

shows the type/ # of atoms in the smallest representative unit of a compound

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5
Q

formula unit:

A

the simplest whole # ratio of ions in an ionic compound

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6
Q

molecular formula:

A

shows the types/ # of atoms combined in a single molecule of a molecular compound

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7
Q

Intramolecular forces:

A

occur between atoms

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8
Q

Intermolecular forces:

A

occur between molecules

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9
Q

Intermolecular forces are not discussed in ionic bonding bc…

A

there are no molecules

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10
Q

The strength of intermolecular forces will affect the properties of:

A

covalent compounds such as melting and boiling points

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11
Q

which one is stronger: intra or intermolecular?

A

INTRAmolecular forces are much stronger

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12
Q

A covalent bond is formed when:

A

two forces balance (cancel out) at the precise distance where potential energy is at a minimum

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13
Q

molecular orbital:

A

shared e- orbital

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14
Q

Lowering potential energy =

A

stability

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15
Q

Most atoms have lower potential energy when they are ________than they have as an_____

A

bonded to other atoms than they have as an independent atom

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16
Q

A bond forms when atoms are…

A

a certain distance from each other

17
Q

bond length:

A

the distance between two bonded atoms at their minimum potential energy

18
Q

bond energy:

A

the energy required to break a chemical bond

19
Q

Forming bonds atoms –>

A

releases energy

20
Q

breaking bonds –>

A

requires (takes) Energy

21
Q

When forming bonds, atoms ________ energy. What amount of energy must be needed to break the bonded atoms?

A

release energy and need the same amnt

22
Q

The shorter the bond length:

A

the more energy required to break it

23
Q

Double bonds/ triple bonds are :

A

stronger (more energy required to break the bonds)

24
Q

The octet Rule:

A

covalent compounds from bonds by sharing e- so each atom has outer energy level with 8 e-

25
Q

shared e-:

A

form overlapping orbitals so that each atom achieves a noble gas configuration

26
Q

Diatomic elements:

A

most stable in pairs and not found as single atom in nature

27
Q

Exceptions to the octet rule:

A
  • atoms that cant fit 8 e- & atoms w/ more than 8 e-
    ex. hydrogen
    boron
    main-group elements in period 3 and below
28
Q

Lewis structure:

A

H-H or :C-C:

29
Q

Resonance:

A

when a single Lewis structure does not clearly represent a covalently bonded molecule or ion
O=S-O <-> O-S=O

30
Q

Bond characteristics:

A

-dont conduct electricity (no ions)
- no partially charged poles (ends)
-low melting/boiling points (bc of weak bonds)
- attraction of polar ends form weak intermolecular forces
- e- orbital overlap = molecular oribtals
-polar covaent -> soulable in water
-nonpolar-> is not