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School > Chemistry Test - Bonding Part II > Flashcards

Chemistry Test - Bonding Part II Flashcards

1
Q

Valence Electron:

A

An electron in the outermost energy level or orbit.

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2
Q

Electronegativity:

A

The ability of an atom to attract bonding electrons to itself.

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3
Q

Covalent Bond:

A

The bond that results from the sharing of a pair of electrons by two atoms.

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4
Q

Polar Covalent Bond:

A

A covalent bond formed between atoms with significantly different electronegativities resulting in a bond with localized positive and negative charges or poles.

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5
Q

Ionic Bond:

A

The electrostatic force of attraction between a positive ion and a negative; a type of chemical bond.

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6
Q

Covalent Range

A

0 to 0.4
For example CH4
C 2.6
H -2.2
= 0.4

Charges: none
Polar or non-polar: non polar covalent

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7
Q

Polar Covalent Range

A

0.5 to 1.7
For example H20
O 3.4
H -2.2
= 1.2
Bond Type: polar covalent
Charges: partial

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8
Q

Ionic Range

A

1.8+
For example LiF
F 4.0
Li -1.0
=3.0
Bond TYpe: Ionic
Full charges

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9
Q

In a polar covalent bond or ionic bond which atom is labelled with a negative symbol?

A

The one with the higher electronegativity.

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10
Q

What symbol do you use to draw a bond dipole?

A

Delta δ+ δ- and that arrow thing.

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11
Q

Lesson #18 - VSEPR Shapes and Polarity
Steps to drawing:

A
  1. Calculate the electronegativity difference
  2. Identify the bond rating (polar-covalent bond)
  3. Identify the charge type (partial charges)
  4. Draw the diagram according to how many of the second molecule, add in the deltas and the dipole
    Identify as polar, non-polar, or non-polar with dipoles that cancel out
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12
Q

Ion - Ion

A

Strongest force of attraction (actually an ionic bond!). Occurs between 2 Ionic Molecules with opposite charges (+1 - 1-) Examples (NaCl, NaBr, KCl, etc).

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13
Q

Ion - Dipole

A

Second Strongest force of attraction. Medium strength. A polar ion and a molecule are attracted to each other. (Like the positive end of a polar water molecule being attracted to salt). (δ+ - 1-)

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14
Q

Hydrogen Bonding

A

Medium strength force of attraction between two dipoles but slightly stronger than dipole-dipole. “Hydrogen Almost Bond.” It happens when F, O, or N atoms are bonded to an H (i.e. HF, H20, or NH3).

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15
Q

Dipole-Dipole

A

A weaker Dipole-Dipole source, the electronegativity difference is smaller, Between covalent polar molecules without an F, O, or N attached to an H. (δ+ - δ-)

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16
Q

London Dispersion Forces

A

The weakest force occurs between non-polar, no charges, molecules. (C-H, C-C)

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17
Q

Order of forces from strongest to weakest:

A
  1. Ion-Ion Bond
  2. Ion-Dipole Force
  3. Hydrogen Bonding Force
  4. Dipole-Dipole Force
  5. London Dispersion Forces
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18
Q

If…
Both particles are ions with full +1, +2, +3 or -1, -2, -3 charge then its…

A

Ion-Ion

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19
Q

If…
One of the particles is a fully charged ion and one is a polar covalent molecule it’s…

A

Ion-Dipole

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20
Q

If…
Both molecules have an H attached to an O,F, or N it’s…

A

Hydrogen Bonding

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21
Q

To distinguish between LDF and Dipole-Dipole?

A

calculate electronegativity if it’s between 0-0.4 it’s LDF, anything higher is Dipole-Dipole

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22
Q

Bigger Dots =

A

Bigger Force so draw Ion-Ion with the biggest dots and LDF with the smallest (Ion-Ion should really be a line)

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23
Q

Dots go from positive to negatice:

A

ions have the charge
O, F, and N are always the negatives, H will be the positive

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24
Q

Melting Points and Structure Format - Wax

A

Wax has non-polar covalent CC and CH bonds with no charges. Therefore, Wax is a non-polar compound with weak LDF forces sticking the molecules to each other. Therefore, little heat is needed to separate the molecules from each other and wax melts first.

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25
Q

Melting Points and Structure Format - Sugar

A

Sugar has polar covalent COH bonds with partial charges. Therefore, Sugar is a polar compound with Upper Medium H-Bond forces sticking the molecules to each other. Therefore, a medium amount of heat is needed to separate the molecules from each other and it melts 2nd.

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26
Q

Melting Points and Structure Format - Salt

A

Salt has ionic NaCl bonds with full charges. Therefore, Salt is an ionic compound with ionic super strong ion-ion forces (bond) sticking the molecules to each other. Therefore, a lot of heat is needed to separate the molecules and it melts 3rd.

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27
Q

Template - Melting Point

A

(Blank) has (non polar covalent/polar covalent/ionic) (what molecules) bonds with (no/partial/full) charges. Therefore, (blank) is a (non-polar, polar, ionic) compound with (weak LDF/medium dipole-dipole forces/upper medium hydrogen bonding forces/strong ion-dipole forces/super strong ion-ion forces) sticking the molecules to each other. Therefore, (little/medium/a lot) of heat is needed to separate the molecules from each other and (blank) melts (1sr/2nd/3rd).

State: Polarity, bond strength and type, description of heat needed to melt substance.

28
Q

The stronger the force of attraction between the molecules the higher the ?. The stronger the force of attraction the more ? ?. The weaker the force of attraction the ? the material melts.

A

Melting point
Heat needed
Faster

29
Q

If it has partial or full charges it typically will ? in water. So, if it’s a ? or ? compound it will dissolve. Otherwise, particles with no charge ? water.

A

Dissolve
Polar or Ionic
Repel

30
Q

Solubility - Wax

A

Non-polar wax has no charges that are not attracted to the partial charges in the polar water. Therefore, the wax molecules will not mix with the water and will not dissolve.

31
Q

Solubility - Sugar

A

Polar sugar has partial charges that are attracted to the partial charges in polar water. Therefore, the sugar molecules will mix with the water molecules and will dissolve.

32
Q

Solubility - Salt

A

Ionic salt has full charges that are attracted to the partial charges in polar water. Therefore, the salt molecules will mix with the water molecules and will dissolve.

33
Q

Template - Solubility

A

(Non-polar/polar/ionic) (blank) has (no/partial/ful) charges that (are not/are) attracted to the partial charges in polar water. Therefore, the (blank) molecules (will not/will) mix with the water and (will not/will) dissolve.

State: polarity, charges.

34
Q

For a substance to conduct electricity in water it must have…

A
  • Ionic bonds
  • Full charges
  • Water solubility (so ion-ion it can’t be strong enough to not let water break the attraction, it must dissolve)
  • Ionic polarity rating
35
Q

Electronegativity determines:

A

Bond type
Charge type
Size of the charges

36
Q

2 Groups of Molecules

A
  1. Non polar covalent molecules
  2. Molecules with Polar covalent bonds and ionic bonds
    (Larger electronegativity differences crate bigger charges, pushing the molecule into the polar covalent or even ionic range)
37
Q

In summation…
Bigger electronegativity leads to ? chargers and ? dipoles.
Smaller electronegativity leads to ? charges and ? dipoles.

A

Bigger charges, bigger dipoles
Smaller charges, smaller dipoles

38
Q

Bigger overall dipoles lead to ? intermolecular forces which lead to ? melting/freezing points and ? boiling/condensation points
Smaller overall dipoles lead to ? intermolecular forces with leads to ? melting/freezing points and ? boiling/condensation points

A

Stronger, higher, higher
Weaker, lower, lower

39
Q

Covalent bonds, no charges, will ? dissolve in water (water is polar) and will ? conduct electricity. Weak London Dispersion forces sticking wax molecules to other wax molecules cause ? melting/boiling points.

A

Not
Not
Low

40
Q

Polar covalent molecules have polar covalent bonds that add up to give an overall dipole. They ? dissolve in water but do ? conduct electricity due to partial charges. They have ? melting points but H-bonding has higher ones because of dipole-dipole and themselves, they have a bigger electronegativity different and thus, are stronger.

A

will
not
medium

41
Q

Ionic compounds ? dissolve in water. Ionic compounds ? conduct electricity in the water. They have the ? Intermolecular force of attraction (Ion-Ion). ? melting and boiling points.

A

Will
Will
Strongest
Highest

42
Q

How strong the force is depends on the kind of attraction (how to say it)

A

Ion-Ion = SUPER STRONG Ion-Ion forces
Ion-Dipole = STRONG Ion-Dipole forces
Hydrogen Bonding = UPPER MEDIUM H-Bond forces
Dipole-Dipole = MEDIUM dipole-dipole forces
London Dispersion Forces (LDF) = WEAK LDF forces

43
Q

What is the electronegativity Difference for Covalent Bonds?

A

0 - 0.4

44
Q

What is the electronegativity Difference for Polar Covalent Bonds?

A

0.5 - 1.7

45
Q

The best description for Polar Covalent Bonds?

A

The electrons are pulled to the more electronegative atom making it partially (-).

46
Q

What is true for compounds with Polar Covalent Bonds?

A

They are polar compounds if the bond dipoles don’t cancel out.

47
Q

What is true for compounds with All covalent bonds?

A

They are non-polar since there are no charges.

48
Q

What is the electronegativity difference between C + O?

A

1.0 Polar covalent bond

49
Q

What is true about the charge of carbon dioxide?

A

There are partial charges with C being more (+) and O being more (-)

50
Q

What is true about the solubility of CO2?

A

It is not very soluble in water since the dipoles cancel and your pop will go flat.

51
Q

Most plastics have CH and CC bonds. It got so hot plastic tables melted. Why?

A

CH and CC bonds are non polar covalent created non polar molecules with weak LDF forces.

52
Q

Lead Acid Car Batteries contain Sulfuric acid dissolved in water. Why is the acid used in the Lead ACid Car batteries?

A

Sulfuric acid ionizes in water to give ions that can carry electrical currents.

53
Q

Propane

A

Non polar covalent, no charges
Weak LDF forces (small dots)
Non-polar

54
Q

Hydrogen perioxide

A

Polar covalent, partial charges
Upper medium hydrogen bond forces (O has rhe delta negative, H delta postive, medium dots)
Polar

55
Q

Salt

A

Ionic, full charges
Ion-Ion bond forces (big dots, both have - and postive charges draw em on)
Ionic

56
Q

Propane has…

A

non-polar covalent CH bonds with no charges. Therefore, Propane is a non-polar compound with weak LDF forces sticking the molecules to each other. Therefore, little heat is needed to separate the molecules from each other and propane melts first.

57
Q

Hydrogen peroxide has..

A

polar covalent OH bonds with partial charges. Therefore, Hydrogen perixode is a polar compound with Upper Medium H-Bond forces sticking the molecules to each other. Therefore, a medium amount of heat is needed to separate the molecules from each other and it melts 2nd.

58
Q

Salt has…

A

ionic NaCl bonds with full charges. Therefore, Salt is a ionic compound with ionic super strong ion-ion forces (bond) sticking the molecules to each other. Therefore, a lot of heat is needed to separate the molecules and it melts 3rd.

59
Q

In order to conduct electricity

A

Ionic bonds
Full charges
Water solubility (so ion-ion it can’t be strong enough to not let water break the attraction, it must dissolve)
Ionic polarity rating

60
Q

Oxygen Diiodide = Polar covalent, partial charges
Will not conduct electricity in water because…

A

Not Ion-Ion
No full charges
Does dissolve in water but that doesn’t really matter now
Not ionic polarity rating
The Oxygen diiodide is polar with partial charges, not an ion-ion bond, but is soluble in water as the partial charges in polar oxygen diiodide are attracted to the partial charges in the polar water. Thus, allowing it to dissolve. However, due to it still not being an ion-ion force bond with full charges or an ionic polarity, it will not conduct electricity in the water.

61
Q

Potassium Nitride = Ionic, Full charges
Will conduct electricity in water because…

A

Ion-Ion
Full charges
Soluble in water
Ionic polarity
The potassium nitride is ionic with full charges, an ion-ion bond, and soluble in water as the full charges in the ionic potassium nitride are attracted to the partial charges in the polar water. Thus, allowing it to dissolve. Due to potassium nitrides’ properties of being an ion-ion, having full charges, having ionic polarity, and being soluble in water, it is able to conduct electricity.

62
Q

Mr. Dragert has a canoe paddle that he made in grade 8. The paddle is coated in an oil based stain to protect the paddle when he is using it in the water. Oil based stains have low melting points, and don’t conduct electricity at all!. What type of compound is an oil based stain? How do you know (Use reasons from this question)? Why is it good at protecting the paddle from the water? (a)

A

The oil based stain is a non polar covalent compound.
I know this because of the properties of the oil based stain…
1) Non polar covalent compounds like oil have low melting points with no charges, making wax a non polar compound with weak LDF forces sticking the molecules to each other. Therefore, little heat is needed to separate the molecules from each other.
2) Only ionic compounds conduct electricity, thus, it further supports the oil based stain being covalent since they cannot conduct electricity.
3) The stain is good at protecting the paddle from the water because the stain repels water and does not dissolve as the water beads off. The only compounds that do not dissolve in water are covalent compounds as they have no charges to be attracted to the partial charges in the polar covalent water. Allowing the oil based stain to not mix with the water and not dissolve.

63
Q

While preparing for his canoe trip, Mr. Dragert mixed some red Gatorade powder in water in his water bottle to drink on the trip. He knew that the Gatorade contained sugar. Being a science teacher, Mr. Dragert did not think Gatorade would conduct electricity since it is sweet. He tested the conductivity of the Gatorade and was surprised to find that it was conductive. Give the type of Compound that sugar is and use it to explain why Mr. Dragert didn’t think Gatorade would conduct and why he was surprised to find that Gatorade conducted electricity. [2]

A

The reason Mr. Dragert didn’t think Gatorade would conduct electricity was because the sugar in Gatorade is a polar covalent compound with partial charges. However, in order to conduct electricity the compound has to have an ionic bond, ionic polarity, full charges, and be soluble in water. While the polar dugar is soluble in water due to the partial causes in sugar being attracted to the partial sugar in water and thus, mixing and dissolving, Sugar would be believed not to conduct electricity. This is because it still doesn’t have ionic bonds it has weak LDF forces, it’s not ionic it’s polar, it doesn’t have full charges it has partial. These qualities are needed to conduct electricity in addition to solubility.

64
Q

They say that Gatorade is good at replacing the salt you lose through sweating while being active. Would Gatorade actually contain salt? How do you know given the Conductivity of Gatorade from above? In your answer explain what kind of compound salt is. [2]

A
  • Salt is an Ionic Compound with full charges, allowing it to dissolve in water because the full charges in the ionic salt are attracted to the partial charges in ionic water which lets them mix and dissolve.
  • In comparison to the polar sugar, the ionic salt is qualified to conduct electricity.
  • Salt is an ionic bond between Na and Cl, it is an ionic compound, it has full charades, and is soluble in water.
  • Thus, Gatorade would contain salt because salt can conduct electricity and is good at replacing the salt you lose through sweating.
65
Q

Why do marshmallows need to be roasted over a campfire to melt, leaving them out on the counter will not likely cause them to melt? [2]

A

Leaving marshmallows in the counter will not likely cause them to melt because..
1) They are mainly made of sugar which is a polar covalent compound with partial charges and Upper-Medium strength H-Bonds.
2) In order to break these bonds, a sufficient amount of heat is needed to allow them to melt.
3) Typical room temperature would not be enough to break these bonds and melt the marshmallows which allows you to leave them on the counter without them melting but still melt them with the much more heat that comes from a campfire.

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