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Chemistry > Test 3 > Flashcards

Test 3 Flashcards

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1
Q

Inter Molecular Forces

A

The attractive forces between separate molecules

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2
Q

London Dispersion Forces

A

Attractions between temporary regions of high and low Electron density in noble gases and none polar molecules
This is the weakest of the inter molecular forces.
Sometimes the electrons cluster in a molecule and the clustered electrons on one side have a slight negative charge and the ones on the other side get a slight positive charge

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3
Q

Dipole-Dipole

A

Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule.

Basically it’s a seperation of charges

Attraction between the opposite partial charge in polar molecules

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4
Q

Hydrogen bonding

A

A special type of dipole dipole force between hydrogen and strongly electronegative elements in polar molecules

This one needs N, O, F

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5
Q

Nonpolar Covalent

A

When the electronegativity difference is zero or very this small this means less than .5 Essentially there are equal sharing of the electrons

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6
Q

Ionic bond

A

This is when the electronegativety difference is larger than 2.0 and the complete electronic transfer occurs.
The bonding of a metal and non metal

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7
Q

Polar Covalent

A

This occurs when the electro negativity is in-between .5 and 2.0

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8
Q

What questions should you ask when looking at a lewis structure to figure out is VESPR structure?

A

1) How many things/valence electrons are there around the atom?
2) what structure is the molecule based on?
3) Which atoms are replaced by lone electron pairs?
4) What is the final structure and bond angles?

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9
Q

What is a solution?

A

When the part Solute are dissolved in the particles of the solvent

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10
Q

What is a Solute?

A

Substance that is dissolved

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11
Q

What is a Solvent?

A

The stuff that does the dissolving

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12
Q

What does homogeneous mean?

A

Everything is the same evenly distributive

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13
Q

what is an ionic compound

A

contains ions “metal and a nonmetal,” a lot of them are solids at room temp

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14
Q

What is a molecular compound

A

Contains two nonmetals

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15
Q

Equillbrium

A

When a reactants forward progress (Reactants forming products) is perfectly balanced with the reverse process (products changing into reactants)

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16
Q

Le Chatleirs Principle

A

If stress is place on a system at Equilibrium the system will proceed in a direction that minimizes that stress

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17
Q

Endothermic Reactions

A

Consume Heat

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18
Q

Exothermic reactions

A

Release heat

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19
Q

Molarity

A

The moles of solute per liter of solution

20
Q

What is an acid?

A

Anything that donates a proton?

21
Q

What is a base?

A

Anything that accepts a proton?

22
Q

What does it mean to donate a proton?

A

For the most part it means a Hydrogen Atom without an electron

23
Q

How do you find the charge of a lewis structure?

A

Determine the number of valence electrons that should be present for each atom in the structure.

Count the electrons around each atom in the structure (each lone pair = 2 electrons, each single bond =1 electron, each double bond = 2 electrons, each triple bond = 3 electrons).

Subtract the number of valence electrons that should be present (from step 1) from the electrons counted in step 2 for each atom. This is the formal charge for each atom.

Check that the formal charges add up to equal the overall charge of the molecule.

24
Q

What does formal charge mean?

A

The charge on each atom in a molecule

25
Q

What is he difference between bent and linear?

A

bent has to or more electrons on the central atom of the lewis structure

26
Q

What makes something polar?

A

The furthest thing to the right and highest up Fluorine is the most polar atom

27
Q

Does F-F have a strong polarity?

A

No because they have the same polarity and that cancels out their polarity completely. You want something we a smaller amount of electronagivity. That will give Fluorine a stronger polarity

28
Q

Why is HCl Polar?

A

Because the electrongs are shared unequally

29
Q

polar bond

A

In chemistry, a polar bond is a type of bond between two atoms in which electrons are shared unequally. Because of this, one end of the bond has a fractional negative charge and the other a positive charge. If the bond dipole moments of the molecule do not cancel, the molecule is polar.

30
Q

What are you looking for in a polar molarcule?

A

one pull from one side to the other/ like s strong pul in one given direction

31
Q

Why does polarity happen?

A

Because there is an uneven pull of molecules

32
Q

What is the strongest intermolecular force?

A

Hydrogen Bond

33
Q

Who is Hydrogens Buddies?

A

Nitrogen, Hydrogen, Fluorine

34
Q

In hydrogeny bonding what is the acceptor?

A

the side with the lone pairs

35
Q

In hydrogen bonding what is the doner?

A

The side with the covalent bond

36
Q

What is the difference between polar and nonpolar boiling points?

A

If something is polar it will have a higher boiling point than something that is nonpolar.

37
Q

The strong the intermolecular forces means what?

A

This means a higher boiling point

38
Q

When considering boiling points what determines a strong force?

A

Size of the molecule
The shapes
The types of bonds

39
Q

What bonds have higher boiling points

A

Polar
ionic
hydrogen

40
Q

What bonds have lower boiling points

A

Covalent
london forces
Covalent

41
Q

How does surface area affect the boiling point?

A

The more surface area covered increases the boiling point verse something that covers less area

42
Q

How does the mass of a molecule increase the boiling point of an atom?

A

This creates stronger bonds/more bonds/ and great size making a much higher boiling point

43
Q

The “like dissolves like” principle states that a

substance prefers to dissolve in a solvent that

A 
has the same type of intermolecular forces as 
the substance (polar –vs– nonpolar)
44
Q

What do bases have at the end of their formula?

A

OH

45
Q

What do acids have at the beginning of their formula?

A

H

46
Q

Acid-base reactions always involve the transfer of

A

. a proton from the acid to the base

47
Q

Adding heat to an ice mixture does what?

A

Does not increase heat just melts the ice

Chemistry (5 decks)

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