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AP Chemistry > Unit 2: Molecular and ionic compound structure and properties > Flashcards

Unit 2: Molecular and ionic compound structure and properties Flashcards

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1
Q

Chemical Bonds

A

Attraction between the nucleus of one atom and the electron of another

*There’s a balance between attraction (+, -) and repulsion (+, +)(-, -)

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2
Q

Bond Energy

A

Energy required to break the bond

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3
Q

Bond Length

A

Distance between atoms

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4
Q

Aspects of a single bond

A
  • Fewest shared electrons
  • Weaker attraction between nucleus of one atom and the bonding elements
  • Weaker + Longer bond
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5
Q

Aspects of a Triple Bond

A
  • Most shared electrons
  • Stronger attraction between nucleus of one atom and the bonding electrons
  • Stronger + shorter bond
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6
Q

Ionic Bonds

A

Electrostatic attraction between a cation (positively charged) and anion (negatively charged)

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7
Q

Mg(OH)2 -> Mg^+2 + 2OH-, Lattice Energy: 2900

Sr(OH)2 -> Sr^+2 + 2OH-, Lattice Energy: 2300

Explain why in terms of periodic properties and Coulomb’s law that it takes less energy for Sr(OH)2 to separate its ions in terms of periodic property and Coulomb’s law.

A

Periodic property: The Sr^2+ ion is larger than the MG^2+ because it has more occupied energy shells; the bond length is longer and weaker

Coulomb’s Law: Since the distance between Sr^2+ and OH- is longer than the distance between Mg^2+ and OH-, the attractive forces in Sr(OH)2 are weaker, and its lattice energy is smaller

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8
Q

Electronegativity

A

The ability of an atom in a molecule to attract shared electrons to itself

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9
Q

Ionic bonds (electron definition)

A

Transferring electrons (usually involves a metal and nonmetal)

*think of it as: if the two elements differ in electronegativity, it is more ionic, and the more electronegative atom has more ability to attract or transfer shared electrons

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10
Q

Covalent bonds

A

Sharing electrons (usually two nonmetals)

*think of it as: if two elements have similar electronegativity, covalent electrons share electrons more equally

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11
Q

Nonpolar (covalent bond)

A

Electrons shared equally

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12
Q

Polar (covalent bond)

A

Electrons shared unequally

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13
Q

Metallic bonds

A

Electrons not associated with a atom or molecule (delocalized electrons)

Positive metal ions surrounded by a sea of mobile valence electrons

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14
Q

Bond Polarity

A

Difference in electronegativity values of two elements

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15
Q

δ− (negative partial charge)

A

Atoms with high electronegativity

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16
Q

δ+ (positive partial charge)

A

Atoms with low electronegativity

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17
Q

Dipole arrow points…

A

Towards the more electronegative atom

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17
Q

A student claims that F2 is more polar than H2 because fluorine has a higher electronegativity than hydrogen. Do you agree with this claim?

A

No; Polarity is the difference in electronegativity, not the absolute value of the electronegativity. Fluorine and hydrogen have the same difference in electronegativity (0), so they have the same polarity.

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18
Q

In order to conduct electricity, a substance must have…

A
  • Charged particles
  • particles that are free to move
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19
Q

Alloys

A

Combining two or more metallic elements

20
Q

Substitutional allow

A
  • Atoms of similar radii
  • One atom substitutes for another atom in the lattice
21
Q

Interstitial alloy

A
  • Atoms of different radii
  • Smaller atom fills the spaces between larger atoms
  • Usually the alloy is stronger than the base metal
22
Q

Octet rule

A

All atoms end up with 8 electrons around them

23
Q

Expanded Octet

A

Atoms in periods 3-7 can bond with other atoms in such a way they end up with more than 8 electrons in their octets

They can do this because they have d-orbitals in their outer shells that can accept electrons

24
Q

Formal charge

A

The hypothetical charge the atom would have if all of the atoms had the same electronegativity

Calculated to identify the most stable/likely structure

25
Q

Formal charge formula

A

(# of valence electrons assigned to the neutral atom) - (# of electrons assigned to the atom in the structure)

**bonds count as one!!!

26
Q

The potential energy of valence electrons ___ as they approach the nucleus of another atom

A

Decreases

27
Q

Bond energy is ___ during the formation of a bond

A

Released

28
Q

Potential energy and bond energy has an __ relationship

A

inverse

29
Q

As the # of bonds between 2 atoms increases, the bond length ___ and the bond energy ___

A

Decreases; Increases

30
Q

Bond Order

A

The number of bonds between two atoms

31
Q

Resonance Structures

A

A set of two or more Lewis Structures; occurs when a molecule has at least one double bond

32
Q

VSEPR Theory (Valence Shell Electron Pair Repulsion)

A

Charge clouds repel each other due to Coulombic repulsion- terminal atoms move as far away from each other as much as possible

33
Q

2 Charge clouds, 2 bonds, 0 lone pairs

A

Linear, 180 angle

34
Q

3 charge clouds, 3 bonds, 0 lone pairs

A

Trigonal Planar, 120 angle

35
Q

3 charge clouds, 2 bonds, 1 lone pairs

A

Bent, 120 angle

36
Q

4 charge clouds, 4 bonds, 0 lone pairs

A

Tetrahedral, 109.5 angle

37
Q

4 charge clouds, 3 bonds, 1 lone pairs

A

Trigonal Pyramidal, 107.3 angle

38
Q

4 charge clouds, 2 bonds, 2 lone pairs

A

Bent, 104.5 angle

39
Q

5 charge clouds, 5 bonds, 0 lone pairs

A

Trigonal Bipyramidal, 90 and 120 angle

40
Q

5 charge clouds, 4 bonds, 1 lone pairs

A

Seesaw, 90 and 120 angle

41
Q

5 charge clouds, 3 bonds, 2 lone pairs

A

T-Shaped, 90 angle

42
Q

5 charge clouds, 2 bonds, 3 lone pairs

A

Linear, 180 angle

43
Q

6 charge clouds, 6 bonds, 0 lone pairs

A

Octahedral, 90 angle

44
Q

6 charge clouds, 5 bonds, 1 lone pairs

A

Square pyramidal, 90 angle

45
Q

Rules of best Lewis diagram structure:

A
  • Will have the minimum number of nonzero formal charges
  • If nonzero formal charges must remain, the negative charge must be assigned to the most electronegative atom
  • The sum of all the individual formal charges must add up to the charge of the chemical species
46
Q

6 charge clouds, 4 bonds, 2 lone pairs

A

Square Planar. 90 angle

47
Q

Molecular Geometry rules:

A
  • Molecules composed of only nonpolar bonds are nonpolar, regardless of shape
  • Molecules in which the central atom is symmetrically surrounded by identical atoms are nonpolar, even if the bonds are polar
  • Molecules with asymmetrical shapes that contain any polar bonds are polar overall
48
Q

Symmetrical shapes:

A

Linear (3 atoms), trigonal planar, tetrahedral, trigonal bipyramidal, square planar, octahedral

AP Chemistry (2 decks)

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