2.7 Lewis Diagrams Flashcards

1
Q

Define Valence electrons

A

electrons in the outermost unfilled s and p orbitals of an atom

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2
Q

The # of __ in an atom is equal to the # of boxes on the periodic table from the left edge up to and including the elements box (excluding d orbital electrons)

A

valence electrons

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3
Q

Why doesn’t neon react w/ other elements?

A

extremely stable w/ 8 valence electrons

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4
Q

Representative elements that have the same valence structure have the same __ and similar __

A

– combining capacity
– chemical properties

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5
Q

Define Electronegativity

A

ability of an atom to pull electrons toward itself

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6
Q

What happens when the electronegativities of 2 atoms are quite different from each other?

A

ionic bonding

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7
Q

Define Covalent bonds

A

When atoms share electrons; typically b/w nonmetals

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8
Q

How does the electronegativity in diatomic molecules affect their bonding?

A

are identical; electrons are shared equally

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9
Q

The __ of an element often indicates how many bonds it will form

A

combining capacity

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10
Q

Lone pair vs bonding pair

A

– electron that is paired up
– single electron needing to bond to make a full octet

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11
Q

Structural diagrams represent __ only

A

bonding electrons

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12
Q

Define ‘formula unit’

A

The simplest ratio of ions in an ionic crystal lattice

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13
Q

State the octet Rule and any exceptions

A

– All atoms want to become more stable by gaining a full valence shell of 8 electrons
– H and He are satisfied by only 2 electrons

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