Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

General Chemistry > Chemical Bonding > Flashcards

Chemical Bonding Flashcards

1
Q

covalent bonds

A

break and form new bonds

formed when 2 atoms share electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

non-covalent bonds

A

weak attractions between atoms with different partial charges within dipoles that don’t share electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

van der waals forces

A

london dispersion forces
ionic bonds
hydrogen bonds
hydrophobic interactions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

london dispersion forces

A

induced dipole- induced dipole
occurs when 2 molecules are close together
mutual attraction with weak temporary dipole moment

more pronounced in larger nonpolar molecules because larger electron cloud, so increased polarization

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

ionic bonds

A

salt bridge
2 charged atoms attracted to opposite charges

complete transfer of electrons from atom with low electronegativity to high electronegativity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

dipole-dipole interactions

A

type of noncovalent bond that occurs between polar molecules with a net dipole moment

align in such a way that partial negative charge is pulled toward the partial positive charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

diatomic molecules

A

hydrogen, nitrogen, oxygen, fluorine, iodine, chlorine, and bromine

form covalent bonds to get full outer shell and be more stable

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

polar covalent bond

A

unequal sharing of electrons which creates an electric dipole

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

nonpolar covalent bond

A

equal sharing of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

bond dissociation energy

A

energy required to break a chemical bond

related to the bond length (distance between nuclei of bonded atoms)

shorter bonds are stronger and require more energy to break

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What makes bonds stronger?

A

shorter bonds with small atomic radii

these will be closer to the top of the periodic table because moving toward indicated that another electron shell and therefore a larger atomic radius

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What type of bonds do hydrogen make

A

short strong bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

polar covalent bond

A

unequal sharing of electrons which creates an electric dipole

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

nonpolar covalent bond

A

equal sharing of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

bond dissociation energy

A

energy required to break a chemical bond

related to the bond length (distance between nuclei of bonded atoms)

shorter bonds are stronger and require more energy to break

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What makes bonds stronger?

A

shorter bonds with small atomic radii

these will be closer to the top of the periodic table because moving toward indicated that another electron shell and therefore a larger atomic radius

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What type of bonds do hydrogen make

A

short strong bonds

18
Q

dipole moment

A

occurs when positive charge accumulates at one end of the molecule and negative charge accumulates at the other

the greater the difference in charge, the greater the dipole moment

additive effect: same direction increases dipole moment; opposite direction can cancel out

19
Q

do symmetrical molecules have a net dipole moment?

A

typically no because dipole moments are canceled out by being in opposite directions

20
Q

electron affinity

A

quantitative measure of the energy change when an electron is added to an atom in the gas state

the more negative the change in energy, the more energy released upon addition of electron

21
Q

Why does Oxygen have the lowest electron affinity in the 6A group?

A

oxygen holds its electrons very close to the core which results in greater electron-electron repulsion

22
Q

When an electron is shielded

A

shielding occurs as valence electrons move away from the positive nucleus

electrons can shield each other from the pull of the nucleus, decreases the attraction between the electron and the nucleus as electrons move away from the nucleus

23
Q

Water as a solvent

A

water can dissolve many polar and ionic compounds because can interact well through hydrogen bonding and electrostatic interactions

  • water is more electronegative than hydrogen which results in a dipole interaction - makes water more desirable to interact with
  • bent geometry of water contributes to its polarity by grouping positive charges at one end of the molecule and negative charges at the other
  • water’s small size allows efficient formation of a hydration shell around solutes
24
Q

solvent

A

substance that dissolves a solute, resulting in a solution

25
Q

surface tension

A

force induced between a liquid and a gas
molecules in the liquid interact with each other more strongly than with molecules in the air, causing the surface of the liquid to behave as a thin film

26
Q

What does the freezing point depend on?

A

strength of intermolecular forces

freezing occurs when the kinetic energy of a molecule can no longer overcome the intermolecular forces binding it to nearby molecules

27
Q

colligative properties

A

properties affected by the amount but no the identity of the solute

28
Q

hydrogen bonding

A

strong intermolecular force that occurs between hydrogen atom and an electronegative atom with lone electron pair

can only occur over short distances so require small electronegative atoms –> F, O, N

29
Q

sigma bonds

A

overlap end to end

  • low energy state and very stable because lots of overlap
  • very strong alone
30
Q

pi bonds

A

overlap of p orbitals perpendicularly

  • high energy state and not stable so require less energy to break (small dissociation energy)
  • weak bonds when alone
  • double bonds are strong because there is both a sigma and a pi bond
31
Q

bond length and dissociation

A

the longer the bond length (sigma bonds are long, pi bonds are short), the more energy needed to break the bond

aka the longer the bond length, the more dissociation energy needed

32
Q

disproportionate reaction

A

atoms of the same element undergo both oxidation and reduction

33
Q

Ag oxidation

A

+1

34
Q

Cd oxidation

A

+2

35
Q

Zn oxidation

A

+2

36
Q

Ga oxidation

A

+3

37
Q

Al oxidation

A

+3

38
Q

coordination chemistry - metals

A

metals can act as Lewis acids because they have empty valence orbitals that can readily accept electrons

39
Q

Order that electrons are removed from shell?

A

electrons are removed from the valence electron shell with the greatest principle quantum number first because they electrons are the furthest from the nucleus and therefore the least tightly bound

ex: [Xe]6s^2 4f^7 5d^1

removed would be 6s then 5d then 4f

40
Q

What would happen to the van der waals force if you replaced valine with alanine?

A

the london dispersion force would decrease because valine is a larger molecule and will have a greater electron cloud causing the molecule to be more polarized

replacing it with alanine (smaller molecule) will decrease the interaction

General Chemistry (10 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions