Bonding and Chemical Interactions Flashcards

1
Q

one or more electrons from an atom with a low ionization energy (typically a metal) are transferred to an atom with a high electron affinity (typically a nonmetal), resulting electrostatic attraction between opposite charges holds ions together

A

ionic bonding

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2
Q

an electron pair is shared between two atoms (typically nonmetals) with relatively similar values of electronegativity; degree to which electron pair is shared determines degree of polarity

A

covalent bonding

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3
Q

electron pair is shared equally

A

nonpolar covalent bonding

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4
Q

electron pair is shared unequally

A

polar covalent bonding

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5
Q

if both of the shared electrons are contributed by only one of the two atoms

A

coordinate covalent bonding

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6
Q

form between atoms that have significantly different electronegativities, electrons are not shared, very high boiling and melting points

A

ionic bonds

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7
Q

formed by atom that loses electrons

A

cation

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8
Q

formed by atom that gains electrons

A

anion

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9
Q

structure formed by ionic constituents in a solid state, consists of repeating positive and negative ions

A

crystalline lattice

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10
Q

form between atoms with similar electronegativities, share electrons, lower boiling and melting points

A

covalent bonds

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11
Q

bond with nearly identical electronegativities, equal distribution of electrons, no separation of charges

A

nonpolar covalent bond

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12
Q

bond with atoms that differ moderately in electronegativities, share electrons unevenly, have separation of charges

A

polar covalent bond

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13
Q

a vector quantity of polar bond or molecule

A

dipole moment (p)

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14
Q

dipole moment (p)

A

p = qd

where:
q = magnitude of charge
d = displacement vector separating partial charges

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15
Q

bond where both of shared electrons originated on same atom, such as when lone pair of one atom attacks another atom with an unhybridized p-orbital to form a bond, typically found in Lewis acid-base reactions

A

coordinate covalent bond

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16
Q

resonance structure stability is greater when:

A

1) less or smaller formal charges are present
2) there is less separation between opposite formal charges
3) negative formal charges are placed on more electronegative atoms

17
Q

spatial arrangement of all pairs of electrons around central atom, including bonding and lone pairs of electrons

A

electronic geometry

18
Q

spatial arrangement of only bonding pairs of electrons

A

molecular geometry

19
Q

weak electrostatic interactions between atoms and compounds, can impact boiling and melting points

A

intermolecular forces

20
Q

attractive or repulsive forces of short lived and rapidly shifting dipoles, a type of van der Waals force, weakest type of intermolecular forces

A

London dispersion forces

21
Q

attractive electrostatic force between positive region of one molecule close to the negative region of another, denoted by dashed lines between molecules, present in solid and liquid phases, polar species tend to have higher boiling and melting points, middle strength of intermolecular forces

A

dipole-dipole interactions

22
Q

unusually strong dipole-dipole interaction formed when hydrogen molecules bond to very electronegative N, O, or F; H atom carries very small amount of electron density in covalent bonds allowing it to essentially act as a naked proton interacting with partial negative charges of nearby molecules; very high boiling point, strongest type of intermolecular forces

A

hydrogen bonds