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DAT GenChem > GenChem3 (Bonding and Chemical Interactions) > Flashcards

GenChem3 (Bonding and Chemical Interactions) Flashcards

1
Q

Forces within a molecule that are weaker than the chemical bond but still play an important role in the physical properties of many substances

A

Intermolecular Forces

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2
Q

What is the octet rule?

What are the exceptions?

A

It states that an atom tends to bond with other atoms until it has eight electrons in its outermost shell, to form a stable electron configuration.

Hydrogen, lithium, beryllium, boron, and elements beyond the second row.

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3
Q 
Why is hydrogen an exception to the octet rule?
Lithium?
Beryllium?
Boron?
Elements beyond the 2nd row?
A

Hydrogen can only have 2 valence electrons
Lithium Can only attain 2 valence electrons
Beryllium can only attain 4 valence electrons
Boron can only attain 6 valence electrons
Elements beyond the 2nd row can expand octets to include more than 8 by incorporating d-orbitals

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4
Q

A bond formed when a smaller atom with a smaller ionization energy is transferred to an atom with a greater electron affinity, resulting in ions being held together by electrostatic force

A

Ionic Bond

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5
Q

Type of bonding where an electron pair is shared between two atoms

A

Covalent Bonding

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6
Q

A covalent and partially ionic bond is a

A

Polar covalent bond

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7
Q

When two atoms with large differences in electronegativity react, there is complete transfer of electrons from the less electronegative atom to the more electronegative atom. This is what type of bonding?

A

Ionic Bonding

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8
Q

The atom that loses electrons is the

The atom that gains electrons is the

A

Cation (positively charged)

Anion (negatively charged)

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9
Q

What value must the difference between two electronegativities of two atoms be for ionic bonding to occur?

A

1.7

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10
Q

Elements of group VII often form ionic bonds with groups..

A

I and II

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11
Q

The electrostatic force of attraction between the charged ions is called an…

A

ionic or electrovalent bond

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12
Q

Ionic compounds have HIGH/LOW melting/boiling points

Why?

A

Ionic compounds have high melting/boiling points

Due to the strong electrostatic forces between the ions

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13
Q

Under what circumstances can ionic compounds conduct electricity?

A

Liquid and aqueous state, not the solid state

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14
Q

What structure do ionic solids form, consisting of infinite arrays of positive and negative ions in which the attractive forces between ions of opposite charge are maximized, while repulsive forces between ions of like charge are minimized

A

Crystal Lattice

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15
Q

Covalent compounds are HIGH/LOW melting
Covalent compounds are SOLID/LIQUID/GAS
Covalent compounds CONDUCT/DON’T CONDUCT ELECTRICITY in liquid states

A

Covalent compounds are LOW melting
Covalent compounds are SOLID
Covalent compounds DON’T CONDUCT electricity

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16
Q

Can atoms share more than one pair of electrons?

A

Yes. Duh.

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17
Q

The average distance between the two nuclei of the atoms involved in a covalent bond

As the number of electron shares increases, what happens to this variable?

A

Bond Length

It decreases

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18
Q

The energy that is required to separate two bonded atoms.

A

Bond energy

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19
Q

The shared valence electrons of a covalent bond are called the
The valence electrons that are not involved in the covalent bond are called this, or…

A

Bonding Electrons

Non-bonding Electrons, lone pair electrons

20
Q

Lewis structures represent which orbitals of electrons?

A

s and p valence orbitals

21
Q

Which atom is usually the center atom?

Which atoms usually occupy the end position?

A

The least electronegative atom typically is the center atom

Hydrogen and the halogens typically are on the end position

22
Q

What is the equation for the formal charge of an atom in a molecule?

A

Formal charge = V-1/2N(bonding)-N(Nonbonding)

V=Valence electrons in free atom
N=number of electrons

23
Q

True/False: More stable resonance structures contribute more to the resonance hybrid

A

True!

24
Q

True/False: A Lewis structure with formal charge is preferred to one with no formal charge

True/False: A Lewis structure in which negative formal charges are placed on more electronegative atoms is more stable than one in which formal charges are placed on less electronegative atoms

A

False!

True!

25
Q

True/False: Atoms found in or beyond the third period can have more than eight valence electrons

A

True!

They can be assigned more than four bonds

26
Q

In the sulfate ion (SO4)^-1, how many bonds and valence electrons can sulfur hold?

A

6 bonds, 12 valence electrons

27
Q

Polar covalent bonding occurs between atoms with small differences in electronegativity, what is the range of electronegativity difference (generally)?

A

0.4-1.7 Pauling Units

28
Q

The equation for the dipole moment (u) in polar covalent bonds is

A

u = qr [C*m]

q=product of the charge magnitude
r= distance between two charges

29
Q

This type of covalent bond occurs between atoms that have the same electronegativities, and occurs commonly in diatomic bonds (N2, H2, etc)

A

Nonpolar covalent bond

30
Q

This type of bond occurs when a shared electron pair comes from the lone pair of one of the atoms in the molecule. It is commonly seen in Lewis acid-base compounds

A

Coordinate Covalent Bond

31
Q

What is a Lewis acid?

What is a Lewis base?

A

A Lewis acid accepts an electron pair

A Lewis acid donates an electron pair

32
Q

T/F: A molecule nonpolar bonds is always nonpolar

T/F: A molecule with polar bonds is always polar

A

True!

False! Polar bonds can be arranged in a nonpolar fashion about an atom

33
Q

When two atoms bond to form a molecule, the atomic orbitals interact to form a _______, which describes the probability of finding the bonding electrons.

A

Molecular Orbital

34
Q

If the sign of two atomic orbitals are the same, this is formed

If the sign of two atomic orbitals is different, this is formed

A

Bonding Orbital

Anti-bonding orbital

35
Q

When orbitals overlap head to head, the resulting bond is called a

When orbitals are parallel, a ___ bond is formed

A

sigma bond

pi bond

36
Q

The attractive forces that exist between molecules are collectively known as

Dipole-dipole interactions and dispersion forces are often referred to as

A

Intermolecular Forces

Van der Waals forces

37
Q

Type of intermolecular force where the positive region of one molecule is close to the negative region of another molecule

A

Dipole-Dipole Interaction

38
Q

In what phase do dipole-dipole interactions become negligible?

Why?

A

Gas

The molecules are much farther apart

39
Q

Which tend to have higher boiling points, polar species or nonpolar species?

A

Polar species

40
Q

A specific and unusually strong form of dipole-dipole interaction which may be either intra- or inter molecular. Occurs with hydrogen atoms due to slight positive charge.

A

Hydrogen bonding

41
Q

Do substances that exhibit hydrogen bonding have unusually high or unusually low boiling points?

Why?

A

Unusually high

It is difficult to break the hydrogen bonds

42
Q

Attraction between neighboring molecules resulting from the short lived dipoles created by the random location of covalently bonded electrons within the molecules

A

London Dispersion Forces

43
Q

Dispersion forces are generally STRONGER/WEAKER than other intermolecular forces

When are they most important?

A

Dispersion forces are generally WEAKER than other intermolecular forces

They are most important when molecules are close together, not far apart.

44
Q

The strength of dispersion forces within a given substance depends directly on how easily the electrons in the nucleus can….

Therefore, do larger or smaller molecules possess greater dispersion forces?

A

move aka, be polarized.

Larger molecules have electrons further from the nucleus, so they possess greater dispersion forces

45
Q

The low temperature at which the noble gases liquefy is to some extent indicative of the magnitude of __________ between the two atoms.

It is the only intermolecular force that exists between noble gas atoms.

A

Dispersion forces

DAT GenChem (11 decks)

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