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Pre AP Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

How do you determine if a bond is ionic?

A

The difference between each atom’s electronegativities are 1.7 or greater
OR
There are metals and non metals in the compound

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2
Q

What is a bond?

A

When two nuclei simultaneously attract the same pair of electrons

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3
Q

What are the 3 types of bonds?

A

Ionic, Covalent, and Metallic

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4
Q

How are electrons distributed in an IONIC bond?

A

Transfer of electrons from the metal to the non metal

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5
Q

What happens to the metal and non metal in an ionic bond?

A

The metal becomes a positive cation and the non metal becomes a negative anion

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6
Q

How are electrons distributed in a COVALENT bond?

A

The electrons are shared between the non metals

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7
Q

How can you tell if a bond is covalent?

A

The difference in EN is <1.7
OR
There are two non metals in the compound

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8
Q

How can you tell if a bond is metallic?

A

There are two METALS in the compound

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9
Q

What is a NON POLAR covalent bond?

A
  • The equal sharing of electrons
  • Occurs between two of the same non metal
  • No difference in EN
  • Symmetrical electron distribution
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10
Q

What are partial charges?

A

Partial charges occur when there is uneven sharing of electrons. The atom with greater electronegativity (EN) attracts the electrons more, making it partially negative while the other side is positive because it is losing it’s electrons.

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11
Q

Do partial charges happen in non polar covalent bonds?

A

No, because both atoms have the same EN, so neither atom pulls each other’s electrons.

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12
Q

Do partial charges happen in POLAR covalent bonds?

A

Yes, because the atoms are of different type, making one atom stronger than the other.

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13
Q

What is a POLAR covalent bond?

A
  • Uneven sharing of electrons
  • Non metals of diff types
  • Diff in EN is between 0.4 and 1.7
  • Asymmetrical charge distribution
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14
Q

What is a metallic bond?

A
  • Occurs between two metals

- Electrons float in a sea of mobile electrons

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15
Q

What makes a metals good conductors?

A

Its mobile electrons

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16
Q

Why do atoms pair and lose or gain electrons to do so?

A

To get a full octet (8) valence electrons to make them stable

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17
Q

What process is breaking bonds?

A

Endothermic, because it requires energy to break

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18
Q

What process is forming bonds?

A

Exothermic, because it releases excess energy when the bond is formed

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19
Q

What is a weak bond?

A
  • Takes little energy to break

- Takes little energy to form

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20
Q

What is a strong bond?

A
  • Takes lots of energy to break

- Takes lots of energy to form

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21
Q

For the following equation:

N(g) + N(g) → N2(g) + Energy

is a bond being formed, or broken and is energy being absorbed or released?

A

Formed, Released

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22
Q

What is a non polar MOLECULE

A

when a compounds electron distribution is symmetrical

OCCURS in non polar or polar bonds

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23
Q

What is a polar MOLECULE

A

When a compounds electron distribution is asymmetrical

24
Q

What is a the difference between a polar bond and molecule

A

A polar bond is when two non metals (different) unevenly share electrons. A polar molecule is when atoms shape is asymmetrical.

25
Q

What are the molecular shapes?

A

Tetrahedral, Linear, Bent, Trigonal Pyramidal, Trigonal Planar

26
Q

What are inter molecular forces?

A

Forces BETWEEN molecules holding them together.

27
Q

The strength of IMF increases with:

A

Polarity, Mass, Electron #

28
Q

IMF influences

A

Boiling Pt, Melting Pt, Phase

29
Q

What is hydrogen bonding found between?

A

Found between atoms containing Hydrogen and Fluorine, oxygen or nitrogen.

30
Q

Hydrogen bonding is…

A
  • Not an actual bond, just a force between atoms

- Strongest IMF

31
Q

Examples of hydrogen bonding

A

H2O, NH3

32
Q

What does hydrogen bonding do?

A

Strong hydrogen bonding gives water it’s cohesive properties and high boiling points.

33
Q

The exception to the EN 1.7 rule:

A

Any group 1 or group 2 metal bonded to hydrogen is ionic

34
Q

Polyatomic Ions

A

Some ionic compounds that have more than 2 elements contain polyatomic ions (TABLE E)

35
Q

How to draw molecular (covalent) lewis dot diagrams

A

1: Add an 8 for each element each compound but 2 for H
2: Add up all valence electrons for a second #
3: subtract valence # from octet number
4: Divide by two (that’s # of bonds)
5: Draw and label extra with dots

36
Q

Tip for molecular (covalent) lewis dot diagrams

A

Hydrogen only forms one bond!

37
Q

S
N
A
P

A 
S = symmetrical
N = nonpolar
A = asymmetrical
P = polar
38
Q

High IMF

A

Phase: Solid

39
Q

Low IMF

A

Phase: Gas

40
Q

Vapor Pressure with IMF

A

High IMF : Low VP

Low IMF : High VP

41
Q

Ionic Bonding Facts

A
  • High Melting Pt
  • Hard
  • Conducts electricity as a liquid and aq
42
Q

Why do things conduct electricity in water?

A

They have mobile ions

43
Q

Covalent Bonding Facts

A
  • Low Melting Pt
  • Soft
  • BAD conductivity
44
Q

Metallic Bonding Facts

A
  • High Melting Pt
  • Hard
  • Conduct electricity as a solid and liquid
45
Q

What two elements are liquids?

A

(BrHg)

Bromine and Mercury

46
Q

Do ionic compounds have a shape?

A

NO!

47
Q

Anything with hydrogen bonding has:

A

High boiling pts and cohesive properties

48
Q

Combustion

A
  • Buring something and exothermic

- Water and CO2 produced

49
Q

Synthesis

A

2 or more substances combine to form one larger one

ex: A + B ——-> AB

50
Q

Decomposition

A

A compound is broken down into two or more substances

ex: AB ——> A + B

51
Q

Synthesis and Decomposition are

A

OPPOSITE!

52
Q

Single Replacement

A

Reactants have an element and compound and if the element is more reactive, it will replace one in the compound

ex: AB + C ——> A + BC

53
Q

Double Replacement

A

2 compounds combine and 2 new ones are formed

ex: AB + CD ——-> AC + BD

54
Q

How do you use table J to figure out if single replacement will happen?

A

More active (higher up in scale) will replace less reactive metal in compound

55
Q

What do we use Table F for?

A

To see if a compound is soluble or insolube

Pre AP Chemistry (11 decks)

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