Unit 9- Chemical Bonds Flashcards

1
Q

chem bonds

A

forces that hold the atoms together in substance
- ionic bonding: cation + anion (ionic cpd)(transfer of e-)
- covalent bonding: nonmetal eles (molec cpd)

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2
Q

Lewis Electron-Dot Symbol

A

Symbol of ele surrounded by dots which represent their ve-

  • cations: most have no ve- shown
  • anions: most hve 8 ve-
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3
Q

lattice energy

A

energy required to sep 1 mol of ionic solid into its gaseous ions

LE= (k|Q1Q2|)/r

Q1 and Q2 = ionic charges
r = distance between ions in the solid
- use Q1Q2 for LE but when all the same, use r

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4
Q

covalent bonding

A

results from atoms sharing an e- pair

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5
Q

bond length

A

the distance between the nuclei of 2 bonded atoms

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6
Q

Lewis Structures

A

show how the ve- are arranged in a molec or polyatomic ion

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7
Q

bonding pairs

A

e- shared between 2 atoms and are rep by lines

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8
Q

lone pairs

A

entirely on one atom and are rep by 2 dots

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9
Q

octet rule

A

atoms share e- until each atom is surrounded by 8 e-
- single bond: share 1 pair e-
- double bond: share 2 pair e-
- triple bond: share e pair e-

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10
Q

bond order

A

the # of e- pairs shared between 2 atoms
- as bond order incs, length of bond decs and strength of bond incs

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11
Q

skeleton structure

A

shows which atoms are bonded to each other

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12
Q

central atom

A

bonded to 2 or more other atoms
- usually farthest left and down on periodic table

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13
Q

terminal atom

A

bonded to 1 other atom
* H and F are always terminal

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14
Q

writing Lewis Structure

A
  1. start with the skele structure
  2. sum the ve-
  3. substract 2e- for each bond in skele structure
  4. count the # of e- needed to satisfy octet rule (if # needed > # remain, add 1 bond for each additional 2e- needed )
  5. place remaining e- as lone pairs to satisfy octet rule
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15
Q

bond polarity

A
  • UNEQUAL sharing leads to a POLAR covalent bond
  • EQUAL sharing leads to a NONPOLAR covalent bond
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16
Q

dipole movements

A

measure of the unequal sharing of e-
- zero for nonpolar
- NOT zero fro polar

17
Q

polar covalent bond symbol

A

δ with a +/- to show charges

18
Q

Electronegativity

A

measure of the ability of an atom to attract the shared e- in a chem bond
- inc up and right
H= 2.1
C= 2.5
N= 3.0
O= 3.5
F= 4.0
- diff in electroneg shows if polar or not and comparison to other molecule shows length of arrow. longer = more polar

19
Q

Formal charges

A

a charge assigned to atoms in Lewis structures by assuming the shared e- are divided equally between the bonded atoms

formal charge= # of ve - # of lone pair e - # of bonds

20
Q

comparing Lewis Structures

A
  1. SMALLEST formal charges are FAVORED (more stable)
  2. adjacent atoms w/ formal charges of the SAME sign are much LESS favorable
  3. neg formal charge on MORE electroneg atoms are FAVORED
21
Q

resonance structures

A

differ only in the distribution of the ve-
- indicated by double handed arrow

22
Q

avg structure

A

avg of all resonance structures
- resonance structures contribute equally

23
Q

bond order

A

avg of the bonds
(ex: 1 double bond and 1 single bond = 3/2 = 1.5)

24
Q

electron deficient molec

A

central atoms from Group 2A and 3A do not have enough ve- to complete an octet

25
Q

odd e- molec

A

species with odd # of e-

26
Q

expanded valence shell molec

A

have more than 8e- about an atom in Lewis structure (extra e- on central atom)
- only 3rd period elements or later
- formula: ZFn (where Z= P, S, Cl, As, Se, Br, Te, I, or Xe and Fn= terminal atom)

27
Q

Oxides of heavier elements

A

have a central atom from the 3rd or later periods

28
Q

bond energies (bond dissociation energy)(D)

A

the energy required to break 1 mol of bonds in a gaseous species
- Always endothermic
- deltaH reaction = sum(bond energies of bonds broken) - sum(bond energies of bonds formed)
- lewis structured need to be written
- bond energies (except of diatomics) are avg energies