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General Chemistry > Bonding And Intermolecular Forces > Flashcards

Bonding And Intermolecular Forces Flashcards

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1
Q

Reactivity of covalent and ionic bonds determine…

A

the chemistry of a substance

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2
Q

The physical properties of a substance are determined by

A

the molecular level of the substance

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3
Q

Lewis Dot Structure: electrons in d subshell are not considered

A

valence electrons for transition metals since valence electrons are in the highest n level

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4
Q

Lewis Dot Structure represents?

A

accounts for the number and location of all valence electrons gives the sense of their reactivity

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5
Q

Octet is achieved for what?

A

the stabilize the atom (both of them)

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6
Q

Single Bond?

A

a bond formed from two electrons

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7
Q

Lone pairs are important for

A

determining the structure of the atom, physical properties

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8
Q

Double Bond?

A

four electrons

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9
Q

Triple Bond?

A

six electrons

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10
Q

What is Formal Charge?

A

a way to evaluate a proposed lewis dot structure and determine the sequence of atoms in a compound (when there is more then two atoms in a molecule).
-formal charge tells us if the atoms are sharing their valence electrons in the best way, which is when all charges equal zero.

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11
Q

What is the formula for Formal Charge?

A

FC=V-1/2B-L

V= valence electrons
B= bonded (all the electrons present in the bond)
L= lone pairs
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12
Q

What if the Formal Charge for all possible arrangements of the atoms in not zero?

A

Pick the one with the minimal charges

-the best structures have negative formal charges because more electronegative.

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13
Q

What are Resonance Structures?

A

A more accurate way of showing the electron distribution of atoms when the Lewis Dot Structure fails (this is normally when 2 of the same atoms are around the different center atom and their is one different bond present)
ex. O-S=O
(also shows the formal charge the same in both different ways)

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14
Q

What is a Resonance Hybrid?

A

Shows the two or more resonance structures averaged together because these resonance structures are all occurring at the same time.

  • this is why the bonds (despite being different types) are the same length
  • weighted average, meaning another resonance structure can be less important than the other, this is usually the case when the formal charge is not zero
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15
Q

Resonance structures are two or more structures where:

A. only atom may move around
B. only bonding electrons may move around
C. only nonbonding electrons may move around
D. only nonbonding electrons, and double and triple bonds may move around

A

D (important of ORGANIC)

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16
Q

What is bond length?

A

the distance between two nuclei that are bonded to one another

17
Q

What is Bond Dissociation Energy (BDE)?

A

the energy required to break a bond homolytically (decomposing into two uncharged atoms).

18
Q

What is a Homolytic Bond Cleavage?

A

one electron of the bond is broken and goes to each fragment of the molecule. In this process two radicals (two uncharged atoms) form.
-not the same as Heterolytic Bond Cleavage because while homolytic creates two uncharged atoms, this bond creates charged atoms, anion and cation.

19
Q

What is a Heterolytic Bond Cleavage?

A

(also know as dissociation)

-both electrons of the electron pair that make up the bond end up on the same atom, this forms both a cation and anion.

20
Q

Bond Dissociation Energy is determined by

A

the relationship between bond length and bond dissociation energy

21
Q

What is the trend for Bond Dissociation Energy?

A

the higher the bond order, the shorter and stronger the bond. (single bond=bond order of 1)

22
Q

BDE/bond length comparisons should only be made with what?

A

made with similar bonds (carbon-carbon bonds, carbon-oxgen)

23
Q

(BDE/BOND length) What does it mean for the energy/length of bond when the bond between two atoms that has more s orbitals? More p orbitals?

A

S orbitals- shorter bond length because s is closer to the nucleus, thus more energy.

P orbitals- longer bond length, farther away from nucleus, less energy.

24
Q

What are the different types of bonds?

A

Covalent
polar covalent bonds
coordinate covalent bonds
Ionic bonds

25
Q

What is a covalent bond?

A

formed between two atom when each contributes one or more electrons (unpaired valence electrons).

  • the electrons are shared in order to help both atoms complete their octets.
  • happens between elements that are opposite of each other on the periodic table
26
Q

What are the different types (classes) of covalent bonds and describe them?

A

1) polar covalent bonds: when the electron density is uneven between two nuclei, creating a dipole moment. (due to difference in electronegativity, the greater the electronegativity difference, the more uneven the electron density is, thus greater dipole moment.
2) nonpolar covalent bonds: (usually between two atoms that are the same element or if the difference is very minuscule on the point of ignoring it) electron density between two nuclei are even.

2) coordinate covalent bonds: when the two shared electrons come from only one atom. This creates a Lewis Base (donator of both electrons) also called a ligand, and a Lewis Acid (acceptor of the electrons).
once this bond breaks, the electrons leave with the ligand

27
Q

What does an atom need in order to become a Lewis base/ligand?

A

a pair of nonbonding electrons

28
Q

Carbon atoms with nonbonding electrons are excellent Lewis bases/ligands. Therefore which of the following molecules is NOT a potential Lewis base/ligand?

A. CO2
B. CO
C. CN-
D. CH3

A

A. O = C = O

29
Q

What is an ionic bond?

A

atoms held together by the electrostatic between a cation and anion, where one atom (cation) gives its valence electrons to the other atom (anion) in order to stabilize further.

  • between nonmetal and metal
  • must be a huge difference in electronegativity
30
Q

What determines the strength of the charge of an ion?

A

strength of bond is proportional to the charge of the ions.
-charge decreases as ions get farther apart (meaning ionic radii increase)
-ex. if MgS is Mg= +2 and S= -2
and NaCl is Na= +1 and Cl= -1
then MgS is expected to have a charge that’s four times stronger than the NaCl

31
Q

Which of the following is most likely an ionic compound?

A. NO
B. HI
C. ClF
D. KBr

A

D. KBr

32
Q

What is the VSEPR Theory?

A

It is used to predict the shapes of simple molecules based on examining the nonbonding and bonding electrons.
-pair electrons generally want to be as far away from each other as possible do to repelling each other.

33
Q

Hybridization?

A

model that shows a mathematical combination of atomic orbitals centered on the same atom to produce a hybrid. Most common hybrid is sp hybrid orbital.

34
Q

how much of the s and p orbital are present in sp hybrid?
sp2 hybrid?
sp3 hybrid?

A

50 % s and p
33% s and 67% p
25% s and 75% p

35
Q

How do you determine the hybridization (sp, sp2, sp3) of atoms?

A

type of hybrid= # of attached atoms + # of lone pairs

36
Q

How do you determine the number of hybrid orbitals you have present in a molecule?

A

1+ x (1= s orbital, x=number of p, which can either be 1, 2,3)

37
Q

What is a sigma bond?

A

(present in all bonds) consists of 2 electrons that are between two nuclei. Formed by end-to-end overlap of one hybridized orbital (or s orbital in H’s case) from each atom in the bond.

38
Q

What is a pi bond?

A

(usually only in double and triple bonds) composed of 2 electrons that are localized to the region that lies on opposite sides of the plane formed by the two bonded nuclei and immediately adjacent atoms, not directly between the two nuclei like sigma.
-formed by two unhybridized p orbitals adjacent to each other

39
Q

What types of bonds (sigma or pi) that are present in single bonds?
double?
triple?

A
  1. 1 sigma
  2. 1 sigma, 1 pi
  3. 1 sigma, 2 pi

General Chemistry (11 decks)

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