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chemical bonding Flashcards

1
Q

what is Chemical bonding: how does it occur

A

occurs due to forces of attration that exists between particles

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2
Q

what does chemical bonding help function

A

makes particles function as a unit

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3
Q

what is bond energy

A

the strength of a bond is measured by the amount of energy that is required to break the bond

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4
Q

how does chemcial bonding relate to stability

A

particles become more stable, so they will bond.

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5
Q

when does an endothermic reaction occur (bonds and heat)

A

when we break more bonds than we make, so heat is needed, so it is cooler and cooler.

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6
Q

when does and an exothermic reaction occur (bonds, heat)

A

when we make more bonds than we break, so heat goes out, so the solution gets very hot.

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7
Q

describe the 3 things about ions (electronegativity different) + (who interacts with who) + (electron transfer?)

A

the complete transfer of electrons from one particle to another

difference in electronegativity = greater than 1.67

2 monoatomic ions: metal interacting with non-metal

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8
Q

what happens when ion and covalent compound are in water

A

covalent compounds will remain intact

while: ionic formula units will come apart in water because water is polar.

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9
Q

what is an ion and formula unit

A

the particles that make up an ionic unit are called ions.

the formula unit is the unit that keeps the 2 ions together because of their attraction.

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10
Q

what is the strength of cation and anion

A

the anion is very strongly attracted to the cation.

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11
Q

what is ionic compund

what is the characteristics of ionic compounds

A

the ionic compounds result when ionic bonds form

high melting point, normally water soluble, conductor of electricity in molten state or as aqueous solution, usually form defined crystals

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12
Q

what is a covalent bond

MOLECULE NEVER FORMS WHAT????

A

it involves the sharing of electrons between 2 atoms, and the resulting particles held together by covalent bonds are called molecules.

MOLECULES ARE ONLY IN COVALENT BOND, NEVER AN IONIC BOND

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13
Q

what is the electonegativity difference for non-polar and polar bonds.

A
  1. 0.0-0.4 bond is non-polar
  2. 0.4-1.67 bond is polar, because the one with greatest electronegativity will have more control than the other does; unequal sharing.
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14
Q

what are the several characteristics of molecular compunds

A

non-conductors of elctricity,

low melting points

if it is polar, it is soluble in water, if not polar, it is not soluble

Polar will dissolve polar and nonpolar will dissolve non polar.

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15
Q

Do polar bonds always form polar molecules

A

NOT ALWAYS

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16
Q

single bond

double bond

triple bond

A

one pair of electrons is shared

two pair of electrons are shared

3 pairs of electrons are shared.

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17
Q

what is coordinate covlent bond

A

both elctrons in that shared pair come from same atom, always single bond

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18
Q

are double and triple bonds count as one or more bonds

A

NO, TRIPLE AND DOUBLE BONDS ALWAYS COUNT AS ONE BOND.

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19
Q

what happens with distance for single, double, and triple bond

A

the more -ple/-ble the bond is, the closer the atoms are to each other, so they get harder to break.

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20
Q

can you show coordinate covalent bond structurally,

A

once formed, this coordinate covalent bond, is indistinguishable from others.

in ammonium ion, both electrons from come from nitrogen to form a bond with the hydrogen, so you can’t distinguish it, and you can’t show it structurally.

this is how you draw it on paper.

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21
Q

what does electron dot diagram show

A

Fluorine: 1s22s22p5

7 valence elctrons, unpaired and lone-pair. so the unpaired electrons are available bonding sites. you must ALWAYS FILL THE DIAGRAM ACCORDING TO HUND’s rule

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22
Q

lewis dot structures for ions

A

JUST LOOK AT MY GREEN SHEET WELL

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23
Q

what is the chemical formula of a molecule

A

chemical formula shows tha relative number and kinds of atoms present in a molecule, such as C6H12O6.

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24
Q

what does structural formula do

A

it shows arrangement of atom and bonds

25
Q

what does lewis dot structure show

A

the arrangement of valence electrons in a molecule and whose electrons from what.

26
Q

what does organic structure show

A

arranggements of carbon chains and rings in organic molecules. and it only applies to compounds containing carbon.

27
Q

what is the order of listing in organic structure

A

first carbon, then hydrogen, and then whatever elese is thre.

28
Q

, what is chemical formula and organic structure.

A

C6H6

29
Q

VSEPR, is the acronym for what? and what does it state? any exceptions?

A

valence shell electron pair repulsion theory, it states that electron clouds (orbitals) move as far away from each other as possible in order to minimize repulsion. No exceptions to this theory

30
Q

what is the octate rule, who must follow it?, except who?

A

Everything must follow octate rule, all atoms except H and He must follow octate rule by having a maximum of 8 valence electrons.

31
Q

What does the amount of repulsion determine? Do all clouds repel each other to the same degree. Explain the degrees of Repulsion.

A
  1. Unshared to Unshared
  2. Unshared to Shared
  3. Shared to Shared

lower degree of repulsion as you descend, (in descending order).

Not all clouds repel to each other to the same degree.

AMount of repulsion determines the shape of the molecule

32
Q

look at the green sheet to see how the repulsion of the bonds in a water molecule, specifically the degrees of repulsion

A

look at green sheet

33
Q

what is the hybrid orbital theory

A

it states that in order to create more available bonding positions, sometimes atomic orbitals merge to form _hybrids _and all of which have equaL energy.

34
Q

what are the several types of hybrid orbitals

A

sp = merger of 1s and 1p.

sp2= merging of 1s and 2p orbital

sp3=formed from the merger of 1s and 3p orbital.

sp3d=merge p and 3 orbitals

actually the number of super scripts (on the s it is 1) is equal to the number of bonding sites available for the particle

35
Q

what is resonance

A

sometimes, experimental data does not match the lewis structure- states that sometimes average bond lengths are possible.

You cannot demonstrate it with lewis dot structure, and so experimental data is needed to prove that average bond lengths are possible.

bonds are not necessarrily in one place with lewis dot structure, so it will be in an irregular shape, so the bonds resonate and then rotate around the central atom.

36
Q

what do you draw for resonance diagrams.

show it for benzine

what spreads apart

A

you just draw a bunch of rotating diagrams

you can only show it with structural formula, and you can show benzine with a circle

one pair of electrons spreads itself over 2 locations.

37
Q

linear

A

2 bonds; 0 unshared pair

1 bond; 0 unshared pair

2 bonds; 3 unshared pair

38
Q

angular/ bent

A

2 bond; 2 unshared pair

2 bond; 1 unshared pair

39
Q

trigonal planar

A

3 bond, 0 unshared pair

40
Q

tetrahedral

A

4 bond, 0 unshared pair

41
Q

pyramidal

A

3 bond; 1 unshared pair

42
Q

seesaw

A

4 bond, 1 unshared pair

43
Q

trigonal bipyramid

A

5 bond, 0 unshared pair

44
Q

t-shaped

A

3 bond, 2 unshared pair

45
Q

octahedral

A

6 bond, 0 unshared pair

46
Q

square pyramidal

A

5 bond, 1 unshared pair

47
Q

square planar

A

4 bond, 2 unshared pair

48
Q

what is the hybrid orbital theory exception to? what is it a mix of? who creates the bonding positions? Mixture of what?

A

exception to octate rule, mix of 2 or more types of orbitals (s and p), and unpaired electrons create bonding positions

49
Q

2 bonds; 0 unshared pair

1 bond; 0 unshared pair

2 bonds; 3 unshared pair

A

linear

50
Q

2 bond; 2 unshared pair

2 bond; 1 unshared pair

A

angular/ bent

51
Q

3 bond, 0 unshared pair

A

trigonal planar

52
Q

4 bond, 0 unshared pair

A

tetrahedral

53
Q

3 bond; 1 unshared pair

A

pyramidal

54
Q

4 bond, 1 unshared pair

A

seesaw

55
Q

5 bond, 0 unshared pair

A

trigonal bipyramid

56
Q

3 bond, 2 unshared pair

A

t-shaped

57
Q

6 bond, 0 unshared pair

A

octahedral

58
Q

5 bond, 1 unshared pair

A

square pyramidal

59
Q

4 bond, 2 unshared pair

A

square planar

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