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Chem 20 > chemical bonding > Flashcards

chemical bonding Flashcards

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1
Q

what are the 3 general ways atoms join together

A

ionic
covalent
metallic

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2
Q

what is the purpose of a pew dot diagram

A

to show the valence electrons of an atom

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3
Q

what is ionic bonding

A

non metal bonds with a metal (takes electrons) so all atoms end up with 8 valence electrons

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4
Q

what is covalent bonding

A

non metal bonds with a non metal so all atoms end up with 8 valence electrons

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5
Q

what is metallic bonding

A

two metals that bonded, positive ion in a sea of electrons

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6
Q

which is the weakest bond

A

metallic

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7
Q

what is an ion

A

any atom with more or less electrons than it is supposed to have

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8
Q

what is electronegativity

A

measure of an atoms attraction for another atom’s electrons

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9
Q

what does the electronegativity scale range from

A

0-4

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10
Q

do metals have high or low electronegativity and why

A

low because metals are generally electron givers

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11
Q

do non metals have high or low electronegativity and why

A

high because generally non metals are electron takers

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12
Q

why is electronegativity useful

A

can use the difference between 2 electronegativites and to determine the type of bond

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13
Q

what is the bonding continuum

A

defines how and what compounds bond

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14
Q

what is the electronegativity of a covalent bond

A

less than 1.7

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15
Q

what is the electronegativity of an ionic bond

A

greater than 1.7

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16
Q

steps for lewis structures (covalent bonding)

A

1) determine total # of ve
2) determine central atom (one with the most bonding electrons

3) make bonds with single electrons
- make sure each atom has 8 ve although there are some exceptions

4) count the # of ve in drawing to make sure it is the same as step 1

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17
Q

steps for orbital/electron dot diagrams (ionic bonding)

A

1) show all electrons in an atom with numerical values
2) indicate # of protons in each atom
3) indicate which electrons are transferring to the non metal with an arrow
4) redraw with electrons placed in new spots
5) indicate if each atom is an anion or cation and their charge

+ means lost an electron
- means gained an electron

18
Q

exceptions to the octet rule

A
  • aluminium and boron only need 6 ve

- hydrogen only needs 2 ve

19
Q

what are network solids

A

atoms or molecules held together by covalent bonds

20
Q

steps for lewis structures (polyatomics)

A

1) follow same rules and for
cations: subtract # of electrons from total
anions: add # of electrons to total

21
Q

steps for drawing VESPR shapes

A

1) determine total # of ve
2) determine central atom
3) draw lewis structure
4) determine VESPR shoe and draw
5) label slightly negative side
6) label polarity
7) label intermolecular forces

22
Q

list of VESPR shapes

A 
linear 
trigonal planar
trigonal pyramidal 
tetrahydral 
bent
23
Q

how to determine polarity

A

polar means the central atom is attatched to different atoms

non polar means the central atom is attached to the same atoms

24
Q

exception to determining polarity

A

bent is always polar

trigonal pyramidal is always polar

25
Q

rank the intermolecular forces from least to greatest

A

london dispersion
dipole dipole
hydrogen bond

26
Q

how to identify london dispersion

A

force between non-polars

27
Q

how to identify dipole dipole

A

force between polars

28
Q

how to identify hydrogen bond and trick

A

H-N
H-O
H-F

NOF

29
Q

how to show polarity

A

just write polar or non polar

30
Q

how to determine the slightly negative side

A

atom with the highest electro negativity ( all atoms’ electrons are attracted to this molecule)

31
Q

how to show the slightly negative side

A

weird s symbol kind of a half 8

32
Q

list of diatomics and trick

A 
hydrogen 
nitrogen 
fluorine 
oxygen 
iodine 
bromine

have no fear of ice cold beer

33
Q

how many electrons can the first shell of an atom hold

A

2

34
Q

how many electrons can the second shell of an atom hold and so on

A

8

35
Q

how to determine the valences electrons of an atom

A

group #/ second digit of group #= ve

36
Q

diff rende between trigonal planar and trigonal pyramidal

A

trigonal planar has an atom on top

37
Q

what does a dashed line mean in VESPR shapes

A

atom behind

38
Q

what do a solid triangle mean in VESPR shapes

A

atom in front

39
Q

what for s dashed triangle mean in VESPR shapes

A

atom to the side

40
Q

how to draw VESPR shapes for polyatomics

A

same steps but don’t include polarity or intermolecular force

Chem 20 (5 decks)

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