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Inorganic Chemistry > Chemical Bonding I: Basic Concepts > Flashcards

Chemical Bonding I: Basic Concepts Flashcards

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1
Q

the linking/attraction of atoms to form compounds

A

Chemical Bonding

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2
Q

the outer shell electrons of an atom

A

Valence Electrons

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3
Q

The valence electrons are the electrons that participate in…

A

chemical bonding

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4
Q

___ are also involved in chemical reactions

A

innermost electrons

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5
Q

chemical reactions that involve the nucleus, which produces large amounts of energy.

A

Nuclear Reactions

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6
Q

the tendency of atoms to prefer to have eight electrons in the valence shell

A

Octet Rule

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7
Q

the family not much involved in transferring of electrons but in sharing

A

4A

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8
Q

a representation of the valence electrons of an atom that uses dots around the symbol of the element

A

Lewis Dot Symbol/Structure

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9
Q

pairing starts when there are more than _ electrons

A

4

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10
Q

paired electrons are called…

A

lone pair

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11
Q

cause bonding to have 8 electrons

A

Unpaired Electrons

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12
Q

inactive family because they do not need to bond with other atoms/elements

A

8A

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13
Q

Bonding happens between metals and non-metals.

A

Ionic Bonding

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14
Q

the energy required to completely separate one mole of a solid ionic compound into gaseous ions.

A

Lattice Energy (E)

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15
Q

kilojoules per mole

A

kJ/mol

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16
Q

the temperature where elements melt from being solid to liquid.

A

melting point

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17
Q

More lattice energy =

A

more heat required

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18
Q

a chemical bond in which two or more electrons are shared by two atoms.

A

Covalent Bond

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19
Q

unpaired electrons will be shared to the other unpaired, the process is called ____

A

Covalent Bonding

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20
Q

product of covalent bonding

A

covalent compound

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21
Q

represents sharing

A

dash (-)

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22
Q

Covalent bonds can be single, double, or triple depending on the number of _____

A

sharing

23
Q

two atoms share two pairs of electrons

A

double bond

24
Q

two atoms share three pairs of electrons

A

triple bond

25
Q

refers to the measurement of the radius of the 1st atom to the radius of the 2nd atom.

A

Lengths of Covalent Bond

26
Q

unit of measurement used to measure atomic structures.

A

Picometre (pm)

27
Q

Picometer is ___ of a meter

A

One trillionth

28
Q

More bonds indicate shorter length because if atoms are bonded more times, it becomes __ to each other

A

closer

29
Q

___ = closer = shorter

A

more attraction

30
Q

less bonding =

A

less attraction

31
Q

a covalent bond with greater electron density around one of the two atoms.

A

polar covalent bond or polar bond

32
Q

Polar covalent bond is a covalent bond with ____ sharing of electrions

A

unequal

33
Q

there’s ____ charges in polar covalent bond

A

partial

34
Q

_____ is the region where electrons are being drawn to.

A

Electron rich region

35
Q

______ is the region where electrons are being drawn away from.

A

Electron poor region

36
Q

_____ - indicates that there is partially negative fluorine

A

Sigma negative

37
Q

the ability of an atom to attract ELECTRONS toward itself in a chemical bond.

A

Electronegativity

38
Q

____ has the highest electron affinity.

A

Chlorine

39
Q

____ has the highest electronegativity.

A

Fluorine

40
Q

Electronegativity increases from:

A

Left to right
Bottom to top

41
Q

_____ is a covalent bond with equal electron sharing.

A

Non-polar covalent bond

42
Q

Highest electronegativity difference =

A

Ionic

43
Q

Lowest electronegativity difference =

A

Non-polar

44
Q

a very simplified representation of the valence shell electrons in a molecule

A

Lewis Structure

45
Q

In writing Lewis Structures, draw the _____ of compound showing what atoms are bonded to each other.

A

skeletal structure

46
Q

Put the ___ electronegative element in the center.

A

least

47
Q

Count total number of _____ e-. Add 1 for each negative charge. Subtract 1 for each positive charge

A

valence

48
Q

Complete an octet for all atoms except…

A

hydrogen

49
Q

If structure contains too many electrons, form double and triple bonds on ____ as needed

A

central atom

50
Q

A ____ is one of two or more Lewis structures for a single molecule that cannot be represented accurately by only one Lewis structure.

A

resonance structure

51
Q

The enthalpy change required to break a particular bond in one mole of gaseous molecules is the…

A

bond energy

52
Q

More bond requires more ____ to break it

A

energy

53
Q

Average ____ in polyatomic molecules

A

bond energy

Inorganic Chemistry (7 decks)

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