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Chemistry > Unit 6 > Flashcards

Unit 6 Flashcards

1
Q

Structural formula

A

Graphic representations of the relative placement of atoms in a molecule and the bonds between them

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2
Q

Structural formula AKA

A

Lewis structure

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3
Q

Structural formulas are important to chemists b/c

A

They can predict behavior by knowing the structural formula of molecules

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4
Q

of electrons in a single bond

A

2

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5
Q

of electrons in a double bond

A

4

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6
Q

of electrons in a triple bond

A

6

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7
Q

Bond dissociation energy

A

Total energy required to break the bond between 2 covalent bonded atoms

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8
Q

Is breaking a bond exothermic or endothermic?

A

Endothermic

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9
Q

Forming bonds

A

Exothermic

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10
Q

Longest to shortest covalent bonds

A

Single, double, triple

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11
Q

Strongest to weakest bonds

A

Triple>double>single

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12
Q

Dispersion involves

A

Temporary dipoles

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13
Q

Dispersion occurs between

A

Non polar molecules

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14
Q

Dispersion strength of attraction

A

Low

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15
Q

Dipole-dipole involves

A

Permanent dipoles

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16
Q

Dipole dipole occurs between

A

Polar molecules

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17
Q

Dipole dipole strength of attraction

A

Medium

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18
Q

H bond involves

A

Permanent dipoles of H, N, O, F

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19
Q

Hydrogen bonding occurs between

A

Polar molecules

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20
Q

H bond strength of attraction

A

High

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21
Q

Strength of bonds including ionic

A

Ionic >hydrogen>dipole dipole>dispersion

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22
Q

Three types of polarities

A

Ionic, polar covalent, non polar covalent

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23
Q

Determination of bond polarity

A

The different between the electronegativity of the atoms. If result is between 0.4-1.7, bond is polar covalent

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24
Q

Ionic bonds are always

A

Polar bonds

25
Q

Ionic bond electronegativity

A

Difference greater than 2

26
Q

Non polar covalent bonds have ____ to ____ electronegativity

A

Very low to no

27
Q

All diatomic molecules are

A

Nonpolar

28
Q

Diatomic molecules

A

Br2, I2, N2, Cl2, H2, O2, F2

29
Q

In nonpolar molecules, the dipoles

A

Cancel each other

30
Q

2 molecular shapes that will always produce polar molecules

A

Bent, trigonal pyramidal

31
Q

Intermolecular forces

A

Attractive forces between molecules.

32
Q

Intermolecular forces are much weaker than

A

Intramolecular forces

33
Q

What types of forces/bonds are breaking when water boils?

A

Intermolecular

34
Q

What determines whether particles that make up a substance are solids, liquids or gases?

A

The magnitude (and type) of intermolecular forces.

35
Q

Weaker than ionic bonds

A

Covalent

36
Q

Low meting and boiling points

A

Covalent

37
Q

Generally soft and wont shatter

A

Covalent

38
Q

Poor conductors of heat and electricity

A

Covalent

39
Q

Most are soluble in water

A

Covalent

40
Q

Solid, liquid, gas at room temperature

A

Covalent

41
Q

Strong bonds

A

Ionic bond

42
Q

High melting and boiling points

A

Ionic bond

43
Q

Hard and brittle (solid at room temperature)

A

Ionic bond

44
Q

Poor conductors in solid state

A

Ionic bond

45
Q

Good conductors when molten or dissolved in water

A

Ionic bond

46
Q

Soluble in water

A

Ionic bond

47
Q

Malleable and ductile

A

Metallic bonds

48
Q

Metallic bonds

A

Solid, high melting points, strong bonds

49
Q

Isotope

A

If a compound begins with hydrogen

50
Q

To name an acid that has no oxygen, the prefix is ___ and the acid name ends in ___

A

Hyrdo, ic

51
Q

To name an acid that has oxygen if the compound name ends in -it’s, acid form of the name would end in

A

Ous

52
Q

Electrons are ____ in covalent compounds

A

Shared

53
Q

The tendency of an atom in a compound to attract electrons

A

Electronegativity

54
Q

A kind of bond in which there is unequal sharing of electrons

A

Polar covalent

55
Q

Any bond in which there is electron sharing

A

Covalent bond

56
Q

The particle formed when 2 or more atoms bond covalently

A

Molecule

57
Q

Model that shows how atoms are arranged in a molecule

A

Structural formula

58
Q

Model used to determine the molecular shape

A

VSEPR model

Chemistry (11 decks)

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