General chemistry 3: bonding and chemical interactions

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26 Terms

1
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A/an [...] bond is the sharing of electrons between two elements

covalent

  • between same element

<p>covalent </p><ul><li><p>between same element </p></li></ul><p></p>
2
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[...] bonds are when a single atom provides both bonding electrons

coordinate covalent

  • most often found in lewis acid-base chemistry

<p>coordinate covalent </p><ul><li><p>most often found in lewis acid-base chemistry </p></li></ul><p></p>
3
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[...] bonds are formed by the complete transfer of valence electron(s) between atoms

ionic

  • usually formed between an element with a low ionization energy and an element with a high electron affinity

<p>ionic </p><ul><li><p>usually formed between an element with a low ionization energy and an element with a high electron affinity </p></li></ul><p></p>
4
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[...] refers to the number of bonds between two atoms (single, double, or triple bond)

bond order

<p>bond order </p>
5
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The greater the number of bonds (bond order) the [higher or lower] the bond strength and the [longer or shorter] the bond

higher, shorter bond length

<p>higher, shorter bond length </p>
6
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Non-polar bonds have a △EN that is [...]

less than 0.5

<p>less than 0.5 </p>
7
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Polar bonds have a △EN that is between [...] and [...]

0.5 and 1.7

<p>0.5 and 1.7 </p>
8
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Cations are ions with a [...] charge

positive

<p>positive </p>
9
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Anions are ions with a [...] charge

negative

<p>negative </p>
10
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[...] are large, organized arrays of ions

crystalline lattices

  • ex: solid carbon

<p>crystalline lattices </p><ul><li><p>ex: solid carbon </p></li></ul><p></p>
11
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Hydrogen bonds are most often formed between hydrogen and the following elements: [...]

O, N and F

O-H, N-H, F-H

<p>O, N and F </p><p><span>O-H, N-H, F-H</span></p>
12
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Van der Waals Forces is a general term that includes [...] forces and [...] forces

  • dipole-dipole forces

  • london dispersion forces

<ul><li><p>dipole-dipole forces</p></li></ul><ul><li><p>london dispersion forces </p></li></ul><p></p>
13
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[...] forces are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule

Dipole-dipole

<p>Dipole-dipole </p>
14
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[...] forces are temporary attractive forces created when a temporary dipole induces a dipole in a neighboring molecule

london dispersion forces

  • the weakest intermolecular force

<p>london dispersion forces </p><ul><li><p>the weakest intermolecular force </p></li></ul><p></p>
15
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Place in order of strength:

hydrogen bonds, dipole-dipole forces, and London dispersion forces

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16
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[...] bonds are formed by head-on overlapping between atomic orbitals

sigma

<p>sigma</p>
17
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[...] bonds are formed by lateral (side-by-side) overlap of atomic orbitals

pi

  • the 2nd and 3rd bond in double and triple bonds are pi bonds

<p>pi </p><ul><li><p>the 2nd and 3rd bond in double and triple bonds are pi bonds </p></li></ul><p></p>
18
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[...] is the charge given to an individual element within a molecule

formal charge

<p>formal charge </p>
19
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Give the formula for formal charge

Formal Charge = [...]

Formal Charge = valence electrons − dots − sticks

 

"Dots" are nonbonding electrons 

"Sticks" are pairs of bonding electrons

<p>Formal Charge = <span style="color: mediumseagreen"><strong>valence electrons&nbsp;− dots − sticks</strong></span></p><p>&nbsp;</p><p>"<strong>Dots</strong>" are nonbonding electrons&nbsp;</p><p>"<strong>Sticks</strong>" are pairs of bonding electrons</p><p></p>
20
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<p>O is the hydrogen bond <span style="color: mediumseagreen"><strong>[acceptor or donor]</strong></span></p><p>N is the hydrogen bond <span style="color: mediumseagreen"><strong>[acceptor or donor]</strong></span></p>

O is the hydrogen bond [acceptor or donor]

N is the hydrogen bond [acceptor or donor]

acceptor

donor

  • the acceptor mist possess a lone electron pair

  • the donor is usually strong electronegativity

<p>acceptor</p><p>donor </p><ul><li><p>the acceptor mist possess a lone electron pair</p></li><li><p>the donor is usually strong electronegativity </p></li></ul><p></p>
21
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The bond angle of an sp hybridized atom is [...]

180

<p>180 </p>
22
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The bond angle of an sp2 hybridized atom is [...]

120

<p>120</p>
23
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The bond angle of an sp3 hybridized atom is [...]

109.5

<p>109.5</p>
24
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Bond angles of an sp3d hybridized atom are [...] and [...]

90 and 120

<p>90 and 120 </p>
25
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The bond angle of an sp3d2 hybridized atom is [...]

90

<p>90 </p>
26
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An H2O molecule is a bent because [...]

the lone pair of the electrons repulse each other and push the H atoms away

<p>the lone pair of the electrons repulse each other and push the H atoms away </p>