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School > Chemistry: Chapter 8 > Flashcards

Chemistry: Chapter 8 Flashcards

1
Q

define covalent bond

A

a bond formed when electrons are shared between atoms

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2
Q

define molecule

A

a neutral group of atoms joined together by covalent bonds

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3
Q

define diatomic molecule

A

a molecule consisting of two atoms

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4
Q

define molecular compound

A

a compound that is composed of molecules

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5
Q

define molecular formula

A

a chemical formula of a molecular compound that shows the kinds and numbers of atoms present in a molecule of a compound

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6
Q

define single covalent bond

A

a bond formed when two atoms share a pair of electrons

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7
Q

define structural formula

A

a chemical formula that shows the arrangement of atoms in a molecule or a polyatomic ion

each dash b/t a pair of atoms indicates a pair of shared electrons

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8
Q

define unshared pair

A

a pair of valence electrons that Is not shared between atoms

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9
Q

define double covalent bond

A

a bond in which two atoms share two pairs of electrons

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10
Q

define triple covalent bond

A

a covalent bond in which three pairs of electrons are shared by two atoms

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11
Q

define coordinate covalent bond

A

a covalent bond in which one atom contributes both bonding electrons

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12
Q

define polyatomic ion

A

a tightly bound group of atoms that behaves as a unit and has a positive or negative charge

ex. NH4^+ or SO3^2-

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13
Q

define bond dissociation energy

A

the energy required to break the bond b/t two covalently bonded atoms

usually expressed in kJ per mol of substance

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14
Q

define resonance structure

A

one of the two or more equally valid electron dot structures of a molecule or polyatomic ion

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15
Q

define molecular orbital

A

an orbital that applies to the entire molecule

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16
Q

define bonding orbital

A

a molecular orbital that can be occupied by 2 electrons of a covalent bond

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17
Q

define sigma bond

A

a bond formed when 2 atomic orbitals combine to form a molecular orbital that is symmetrical around the axis, which connects two atomic nuclei

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18
Q

define pi bond

A

a covalent bond in which the bonding electrons are most likely to be found in sausage-shaped regions above and below the bond axis of the bonded atoms

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19
Q

define tetrahedral angle

A

a bond angle of 109.5 degrees that results when a central atom forms four bonds directed toward the center of a regular tetrahedron

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20
Q

define VSEPR Theory

A

valence-shell electron-pair repulsion theory: because electron pairs repel, molecules adjust their shapes so that valence electron pairs are as far apart as possible

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21
Q

define hybridization

A

the mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals

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22
Q

define nonpolar covalent bond

A

a covalent bond in which the electrons are shared equally by the two atoms

23
Q

define polar covalent bond (polar bond)

A

a covalent bond between atoms in which the electrons are shared unequally

24
Q

define polar molecule

A

a molecule in which one side of the molecule is slightly negative and the opposite side is slightly positive

25
Q

define dipole

A

a molecule that has two poles, or regions, with opposite charges

26
Q

define van de waals forces

A

the two weakest intermolecular attractions - dispersion interactions and dipole forces

27
Q

define dipole interaction

A

intermolecular forces resulting from the attraction of oppositely charged regions of polar molecules

28
Q

define dispersion force

A

attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces

these are the weakest interactions between molecules

29
Q

define hydrogen bond

A

attractive forces in which a hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom

30
Q

define network solid

A

a solid in which all of the atoms are covalently bonded to each other

31
Q

what information does a molecular formula provide?

A

it shows how many atoms of each element a substance contains

32
Q

what representative units define molecular compounds and ionic compounds?

A

molecular compounds = a molecule

ionic compounds = formula unit

33
Q

what is the result of electron sharing in covalent bonds?

A

to attain the electron configuration of a noble gases

atoms also form double or triple covalent bonds if they can attain a noble gas structure by sharing two pairs or three pairs of electrons

34
Q

how are coordinate covalent bonds different from other covalent bonds?

A

in a coordinate covalent bond, the shared electron pair comes from one of the bonding atoms

35
Q

what are some exceptions to the octet rule?

A

the rule can’t be satisfied in molecules whose total number of valence electrons is an odd number

there are molecules in which an atom has less, or more, than a complete octet of valence electrons

36
Q

how is the strength of a covalent bond related to its bond dissociation energy?

A

a large bond dissociation energy corresponds to a strong covalent bond

37
Q

how are resonance structures used?

A

chemists use resonance structures to envision the bonding in molecules that cannot be adequately described by a single structural formula

38
Q

how are atomic and molecular orbitals related?

A

just like an atomic orbital belongs to a particular atom, a molecular orbital belongs to a molecule as a whole

39
Q

what do scientists use the VSEPR theory for?

A

to explain the 3-D shape of molecules

40
Q

in what ways is orbital hybridization useful in describing molecules?

A

it provides information about both molecular bonding and molecular shape

41
Q

how do electronegativity values determine the charge distribution in a polar bond?

A

more electronegative atoms attract electrons more strongly and gains a slightly negative charge

the less electronegative atom has a slightly positive charge

42
Q

what electronegativity difference range applies to nonpolar covalent bonds?

A

0.0-0.4

43
Q

what electronegativity difference range applies to moderately polar covalent bonds?

A

0.4-1.0

44
Q

what electronegativity difference range applies to very polar covalent bonds?

A

1.0-2.0

45
Q

what electronegativity difference range applies to ionic bonds?

A

≥ 2.0

46
Q

how do the strengths of intermolecular attractions compare with ionic and covalent bonds?

A

intermolecular attractions are weaker than either ionic or covalent bonds

47
Q

why are the properties of covalent compounds so diverse?

A

because of widely varying intermolecular attractions

48
Q

characteristics of ionic compounds? (7)

representative unit?
bond formation?
type of elements?
physical state?
melting point?
solubility in water?
good/bad conductors of electric current?
A
  1. the representative unit is a formula unit
  2. the bond formation is a transfer of electrons
  3. the type of elements are metallic and nonmetallic
  4. the physical state is a solid form
  5. the melting point is very high
  6. the solubility in water is usually high
  7. they are good conductors of electric current
49
Q

characteristics of molecular compounds? (7)

representative unit?
bond formation?
type of elements?
physical state?
melting point?
solubility in water?
good/bad conductors of electric current?
A

1 molecule

  1. sharing electrons b/t atoms
  2. nonmetallic
  3. solid, liquid, or gas
  4. low
  5. high to low
  6. poor to nonconductors
50
Q

where are the electrons in covalent bonds?

A

in molecular orbitals - atomic orbitals that supply an area for electrons to be shared

51
Q

difference between linear and bent shapes?

A

linear doesn’t have any lone paired electrons; lone paired electrons make the linear shape bend, therefore, it’s bent

52
Q

Weakest electronegative element?

What is it’s value?

A

Cesium - 0.7 –> Least tendency to attract electrons

53
Q

Strongest electronegative element?

What is it’s value?

A

Fluorine - 4.0 –> has strong tendency to attract electrons

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