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Chem > Chapter 7&8 > Flashcards

Chapter 7&8 Flashcards

0
Q

What is a chemical bond?

A

Most bonds are formed because positive atoms are attracted to negative atoms.

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1
Q

What is a Lewis structure?

A

Representation of an atom or ion where the symbol represents the nucleus and all but the valence hell electrons.

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2
Q

Metals are usually____. Nonmetals are usually_____. An exception?

A

Positive
Negative
Hydrogen

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3
Q

What are the three types of chemical bonding?

A

Ionic
Metallic
Covalent

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4
Q

What is ionic bonding?

A

Anions(negative ions) and cations(positive ions) are held together because opposite charges attract.
1 metal/metalloid and 1 nonmetal

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5
Q

Bonds are formed through the___ of electrons.
Metals____ electrons.
Nonmetals____electrons.

A

Transfer
Donate
Accept

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6
Q

Metallic bonds?

A

Electrons are free to move through the solid.
Metals conduct electricity.
2 metals/metalloids

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7
Q

Covalent bonds?

A

Share valence electrons with each other. Both atoms get to count electrons.
2 nonmetals

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8
Q

How does h2 form?

A

Positive nuclei repel each other. Electrons are attracted to positive nuclei atoms share the electrons.

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9
Q

What is a structural formula?

A

Using a line to indicate bonds.

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10
Q

Properties of inorganic and organic compounds

A

N

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11
Q

What is the octet rule?

A

Most atoms try to get right total electrons when bonding.

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12
Q

What are the exceptions to the octet rule?

A

H and He want two electrons
Boron group only wants six
Big Five: S, P, Cl, Br, and I(only when in the middle if the molecule)
Noble gases can exceed octet.

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13
Q

Multiple bonds?

A

Share more than one pair of valence electrons.
Double bond- 2 pairs 4 electrons
Triple bond- 3 pairs 6 electrons

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14
Q

Special rules for Lewis structure?

A

Positive- remove paired electron from center atom

Negative- extra electron from a negative charge pair with an outer atom vacancy(most times)

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15
Q

Special rule for nitrogen Lewis structure?

A

As last resort move electron from center atom to outer atom vacancy.
Final structure must have no completely unpaired electrons n

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16
Q

Beyond octet rule?

A

Rules are same except center atom all electrons can bond.

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17
Q

Lewis structure if acid?

A

Draw polyatomic ion first and attach hydrogen as needed.

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18
Q

VSEPR

A

Number of atoms and line pair electrons predict molecular arrangement.
Number of atoms predict molecular geometry/shape.

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19
Q

VSEPR Arrangement/Shape

A 
AXbEy
A-central atom
X other atoms
E non bonding electron groups
B and y indicate how many of each kind are present
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20
Q

Formal charge equation

A

of outer electrons-(1/2) #bonded electrons- # of line electrons

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21
Q

Resonance

A

Only for covalent bonds.
No complete rotations of atom are allowed.
Move e in same direction.
Charge is conserved.
True structure is mix of all resonance structures. Hybrids

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22
Q

Polar bonds

A

Some differences in electro negativity between atoms. Some bonds are more polar than others.

23
Q

Nonpolar bonds

A

Little to no electro negativity differences between atoms.

24
Q

Polar covalent bond

A

Unequal sharing of the bonding electrons of a covalent bond.
More electronegative aim acquires a partial negative charge(-) less electronegative acquires a partial positive charge(+)

25
Q

Molecular polarity

A

Determined by the arrangement of the molecule.
Symmetrical molecules are nonpolar.
Non symmetrical molecules are polar.

26
Q

Some molecules can individual polar bond however the molecule itself is nonpolar

A

.

27
Q

Dipole moment

A

Adding the vectors(the dipoles) shows the overall direction for polarity of the molecule. Vectors cancel when equal.

28
Q

Hybridization

A

Involves taking individual orbitals and mix them to make combinations

29
Q

Arrangement hybridizations

A 
Linear sp+2p
Trig planar sp^2+p
Tetrahedral sp^3
Trig bipyramidal dsp^3
Octahedral d^2sp^3
30
Q

Carbon hybridization

A

All single bonds sp3
One double bond sp2+p
One triple bond sp+2p

31
Q

Classifications of hydrocarbons

Contains only carbon and hydrogen

A

Alkalane sp3
Alkenes sp2+p
Aromatics sp2+p
Alkynes sp+2p

32
Q

Molecular orbit theory

A

Electrons are assumed to be in hybrid orbitals. Orbitals have different phases. Predicts overall stability of the molecule.

33
Q

What are the three types of molecular orbitals

A

Binding orbitals
Nonbonding orbitals
Antibonding orbitals

34
Q

Bonding orbitals

A

When two orbitals from different atoms actually combine.
Single bond- sigma
Multiple bond - pi
Lowest in energy of the three types.

35
Q

Non bonding orbitals

A

Orbitals that are the atoms line electrons.same energy as starting electrons.
Middle energy if 3 types

36
Q

Antibonding orbitals

A

When two orbitals from different atoms don’t combine.
Highest in energy of the three types.
Single bonds - sigma*
Multiple bonds - pi star

37
Q

Non bonding electrons go somewhere else and all outer electrons matter

A

.

38
Q

Bond order

A

Larger bond order means greater bond strength.

Bond order= # bonding e- # anti bonding e/ 2

39
Q

Intermolecular forces

A

Attractive forces between molecules

Much weaker than chemical bonds within molecules.

40
Q

Three types of IMF

A

London dispersion forces
Dipole dipole forces
Hydrogen bond

41
Q

London dispersion forces

A

Attraction between two instantaneous dipoles.
Asymmetrical electron distribution.
Force for all atoms and molecules.

42
Q

Dipole dipole forces

A

Attraction between two permanent dipoles.
Force for all polar molecules.
Stronger when molecules are closer together.
Medium IMF strength

43
Q

Hydrogen bonding

A

Attraction between molecules with NH oh fh bonds.
Extremely polar bonds.
Very strong dipole dipole force.
Strongest IMF strength.

44
Q

Why does ice float

A

Because it is 9% less than liquid water.

Water becomes denser as it cools until it reaches 4C. Then becomes less dense.

45
Q

Ice

A

Less dense because of its open lattice structure compared to water.
As molecules slow down they arrange themselves into honey comb shaped crystals behold together by hydrogen bonds.

46
Q

Ice

A

10% greater volume than water.
Water freezes from top down.
Later of ice on pond acts as insulator for water below.
Great deal of energy to turn solid water to liquid water.

47
Q

Four types of water properties

A

Surface tension
Capillary action
Solvent
Collimating properties

48
Q

Surface tension

A

Glass of water bulges over top. Water forms round drops because of hydrogen bonds and all molecules on the edge are pulled to the middle. Water molecule can bond 4 times.
All liquids have surface tension

49
Q

Why does water have a meniscus when in a glass tube

A

Glass has polar molecules and can hydrogen bond. Water also has polar molecules and water curves up alongside the glass causing the meniscus.
Hg is nonpolar which causes reverse meniscus

50
Q

How to decrease surface tension

A

Use a surfactant(surface active agent) like detergent or soap. Interfere with hydrogen bounding.

51
Q

How does soap clean grease?

A

Soap has a polar head. Tail(nonpolar) dissolves nonpolar grease in polar water. Forms micelle around grease.

52
Q

Capillary action

A

Attractive force between the surface of a liquid and the surface of a solid.
Driving force or coffee filter experiment.

53
Q

Solution

A

Homogeneous mixture mixed molecule by molecule

54
Q

Solvent

A

Dissolving medium

55
Q

Solute

A

Dissolved particles

56
Q

Aqueous solution

A

Solution with water as the solvent.
Water dissolves ionic compounds and polar covalent molecules best.
Like dissolve like.
Ex. Oil is nonpolar. Oil and water don’t mix. Salt is ionic makes salt water.

Chem (5 decks)

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