Chapter 2 interatomic bonding Flashcards

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1
Q

Some of the following properties are determined by electronic structure

A
  • chemical
  • electrical
  • thermal
  • optical
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2
Q

an atom contains 3 thongs

A

electrons

protons

neutrons

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3
Q

atomic number

A
  • number of protons in the nucleus of an atoms

-

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4
Q

what is an amu?

A

atomic mass number 1/12 mass of 12C

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5
Q

atomic weight

A

wt of 6.022 * 1023 molecules or atonms

1 amu/atom = 1 g/mol

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6
Q

2 models of electronic structure

A

Bohr’s model

wave mechanical atom model

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7
Q

in electron structure, electrons have wavelike and particle properties. two of the wavelike characteristics are

A
  • electrons are in orbitals defined by a probability
  • each orbital at discrete energy level is determined by quantum numbers
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8
Q

quantum number

n =

l =

m<em>l = </em>

ms =

A

n = principal ( energy level shell, size, average distance)

l = subsidiary (subshell, shape)

m<em>l = </em>magnetic (number of obitals)

ms = spin

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9
Q

electron energy states

A
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10
Q

electron states filling orbitals

A
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11
Q

electron configurations

A
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12
Q

* quick reminder *

survey of elements

A
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13
Q

valence electrons

A

those in unfilled shells

are the most available for bonding and tend to control the chemical properties

ex

1s2 2s2 2p2

valence electrons

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14
Q

* quick reminder *

the periodic table

A
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15
Q

electronegativity

A

is a measure of an atom’s ability to attract shared electrons to itself.

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16
Q

electronegativity on the periodic table

A
17
Q

ionic bond

A

type of linkage formed from the electrostatic attraction between oppositely charged ions in a chemical compound.

18
Q

* quick reminder *

ionic bond

A
19
Q

1) ionic bonding occurs between __ and __ ions
2) requires ____ transfer
3) large difference in ________ required
4) good example is _____

A

1) ionic bonding occurs between + and - ions
2) requires electron transfer
3) large difference in electronegativity required
4) good example is NaCI

Na (metal, unstable ) CI (nonmetal, unstable)

Na (cation,stable) + - CI(anion, stable)

20
Q

* quick reference *

ionic bonding on the periodic table

A
21
Q

cations

A

atom or group of atoms that bears a positive electric charge.

22
Q

anions

A

has more electrons than protons, consequently giving it a net negative charge.

23
Q

electron cloud

A

the system of electrons surrounding the nucleus of an atom.

24
Q

* quick reference *

bond hybrization - carbon

A
25
Q

primary bonding

A

involve sharing or donating electrons between atoms to form a more stable electron configuration

26
Q

* quick reference *

primary bonding

A
27
Q

secondary bonding

A

They are usually formed when an uneven charge distribution occurs, creating what is known as a dipole (the total charge is zero, but there is slightly more positive or negative charge on one end of the atom than on the other

28
Q

* quick reference *

secondary bonding

A
29
Q

* quick refernece *

summary bonding

A
30
Q

Tm

A

melting temperature

31
Q

what is the coefficient of thermal expansion represented by

A

α ( alpha )

32
Q

thermal expansion

A

is the tendency of matter to change in shape, volume, and area in response to a change in temperature

33
Q

types of bonding that occurs

ceramics -

metals -

polymers -

A

ceramics - Ionic & covalent bonding

metals - Metallic bonding

polymers - Covalent & Secondary

34
Q

Large bond energy

large __

large __

small ___

A

Large bond energy

large Tm

large Energy

small α (thermal expansion)

35
Q

Variable bond energy

moderate __

moderate __

moderate ___

A

Variable bond energy

moderate Tm

moderate Energy

moderate α (thermal expansion)

36
Q

Directional Properties

Secondary bonding dominates

small ___

small ___

large ___

A

small Tm

small Energy

large α (thermal expansion)