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CHEM 1309 > Chapter 9 Bonding > Flashcards

Chapter 9 Bonding Flashcards

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1
Q

__________ ___________ are the outer shell electrons of an atom that determines an element’s __________

A

valence electrons, chemistry

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2
Q

compared with nonmetals, the number of valence electrons in metals is generally

A

smaller

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3
Q

________ _________ are almost completely unreactive due to _________ __________

A

noble gases, electron configuration

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4
Q

Main group (A) elements tend to _______ or ________ electrons to become isoelectronic

A

gain or lose

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5
Q

isoelectronic means same __________ _________ configuration as nearest noble gas)

A

valence electron

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6
Q

recall that the 4s orbital fills _______ the 3d orbital in the first row of transition metals

A

before

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7
Q

electrons are always lost from the ______________

A

highest n value

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8
Q

two or more species having the same ___________ but different ____________ is called isoelectronic series

A

electronic configuration, nuclear charges

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9
Q

an _________ __________ is a series of two or more species that have _________ electron configurations but _________ nuclear charges

A

isoelectronic series, identical, different

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10
Q

according to ___________ atoms will gain, lose, or share electrons to acquire eight valence electrons. except for ______

A

octet rule, hydrogen

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11
Q

during ionic bond formation, electrons are _________ from one atom to another

A

transferred

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12
Q

in ionic bonds, metals _______ electrons

A

lose

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13
Q

in ionic bonds, nonmetals __________ electrons

A

gain

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14
Q

during covalent bond formation, electrons are ________ between two atoms.

A

shared

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15
Q

Shared electrons are available to _______ bonding atoms

A

both

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16
Q

sharing leads to _____________ around each atom

A

8 valence electrons

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17
Q

shared electrons =

A

bonds

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18
Q

non-bonding valence electrons=

A

lone pairs

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19
Q

electronegativity is a measure of the tendency of an atom to ________ bonding electrons to itself when it is in a molecule

A

attract

20
Q

the higher the electronegativity (EN) value of an atom in a molecule, the more ________ it attracts the electrons (more e- hungry) in a ___________

A

strongly, covalent bond

21
Q

The difference in EN values makes sharing ________ in a __________

A

unequal, covalent bond

22
Q

Electronegativity increases from _________________ across a ______ and from ______________ for a _______

A

left to right, period —-> , bottom to top (arrow up), group

23
Q

the electrical attraction of an atom for the shared electrons is called the atom’s

A

electron affinity

24
Q

What are the numbers for FONC CL H

A

4, 3.5, 3, 2.5, 3, 2.1

25
Q

the most electronegative elements experience an increase in ____________ and attains a __________________

A

electron density, partial negative charge

26
Q

the less electronegative elements experience an decrease in ____________ and attains a __________________

A

electron density, partial positive charge

27
Q

dipole consists of

A

two points of a positive and negative charge

28
Q

when is a bond nonpolar covalent

A

when there is an electronegativity value of 0, electrons are shared equally by two bonded atoms

29
Q

when is a bond polar covalent

A

when there is an electronegative difference of more than or equal to 0.1 but less than 1.9 between two bonded atoms

30
Q

a bond is ionic when

A

there is an electronegative value of equal to or more than 2.0

31
Q

the greater the electronegativity difference between two bonded atoms, the greater the percentage of

A

ionic character in the bond

32
Q

a molecule is polar

A

when there is an electronegativity difference of more than zero, one region of the molecule is has a small positive charge while the other region has a small negative charge

33
Q

the bonding electrons in a non-polar compound

A

have the same EN value, are shared equally, symmetric

34
Q

Lewis structures

A

they show the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule

35
Q

a lewis structure

A

can be drawn for any covalently bonded molecule

36
Q

BF3 lewis structure

A

boron only gets 6 electrons

37
Q

BeCl2 lewis structure

A

beryllium only gets 4 electrons

38
Q

a single line in a lewis structure represents

A

single bond, shared pair of electrons

39
Q

ionic bonding

A

occurs between a metal nonmetal, cation and ion, group 1 and group 7

40
Q

in an ionic bond the elements

A

transfer electrons

41
Q

what happens to a nonmetal in formation of an ionic bond

A

the nonmetal gains electrons and gets a negative ion

42
Q

n^2 gives you

A

orbitals

43
Q

a nonmetal in an ionic bond

A

gains electrons and forms a negative ion

44
Q

nonmetals want to

A

gain electrons

45
Q

bonds that cant be represented by lewis structures are known as

A

resonance

CHEM 1309 (3 decks)

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