Chemistry Chapter 4,5,6 Test

Lewis Structures

Ch. 6- sp=

Ch. 6- sp=

linear

Ch. 6- sp^2=

trigonal planar

Ch. 6- sp^3=

tetrahedral

Ch. 6- sp^3d=

trigonal bipyramidal

Ch. 6- sp^3d^2=

octahedral

Ch. 4- Group 1 elements have what charge ions

+1

Ch. 4- Group 2 elements have what charge ions

+2

Ch. 4- What are the group 1 +1 elements

Li, Na, K, Rb, Cs

Ch. 4- What are the Group 2 +2 elements

Be, Mg, Ca, Sr, Ba,

Ch. 4- What is the charge of the Group 17 elements

-1

Ch. 4- What is the charge of the Group 16 elements

-2

Ch. 4- What is the charge of the Group 15 elements

-3

Ch. 4- di=

2

Ch. 4- tri=

3

Ch. 4- tetra=

4

Ch. 4- penta=

5

Ch. 4= hexa=

6

Ch 4. hepta=

7

Ch. 4- octa=

8

Ch. 4- nona=

9

Ch. 4- deca=

10

Ch. 4- Noble gas charges=

0

Ch. 4- ide acids=

hydro+anion+ -ic acid

Ch. 4- ate acids=

anion+ -ic acid

Ch. 4- ite acids=

anion+ -ous acid

Ch. 6- any single bond=

1 sigma bond

Ch. 6- any double bond=

1 sigma, 1 pi bond

Ch. 6- any triple bond=

1 sigma, 2 pi bond

Ch. 6- Rotation breaks with these bond types

Pi bonds

Ch. 6- sp^3d orbitals can only form-

when n=3 or higher

Ch. 5- difference in electronegativity=

bond polarity

Ch. 5- the larger the difference in electronegativity-

the more polar the bond

Ch. 5- formal charge equation=

(number of valence electrons) - (number of lone pair electrons) - (number of bonds)

Ch. 5- 2 electron groups=

linear electron geometry

Ch. 5- 3 electron groups=

trigonal planar geometry

Ch. 5- 4 electron groups=

tetrahedral

Ch. 5- 5 electron groups=

trigonal bipyramidal

Ch. 5- 6 electron groups=

octahedral

Ch. 5- trigonal planar molecular geometry=

3 e- groups, 0 lone pairs

Ch. 5- bent molecular geometry=

3 e- groups, 1 lone pair

or

4 e- groups, 2 lone pairs

Ch. 5- tetrahedral molecular geometry=

4 e- groups, 0 lone pairs

Ch. 5- trigonal pyramidal molecular geometry=

4 e- groups, 1 lone pair

Ch. 5- trigonal bipyramidal molecular geometry=

5 e- groups, 0 lone pairs

Ch. 5- see saw molecular geometry=

5 e- groups, 1 lone pair

Ch. 5- t shaped molecular geometry=

5 e- groups, 2 lone pairs

Ch. 5- 5 e- groups, 3 lone pairs=

linear molecular geometry

Ch. 5- octahedral molecular geometry =

6 e- groups, 0 lone pairs

Ch. 5- square pyramidal molecular geometry=

6 e- groups, 1 lone pair

Ch. 5- square planar molecular geometry=

6 e- groups, 2 lone pairs

Ch. 6- 2 e- groups, linear=

sp hybridization

Ch. 6- 3 e- groups trigonal planar=

sp^2 hybridization

Ch. 6- 4 e- groups, tetrahedral=

sp^3 hybridization

Ch. 6- 5 e- groups, trigonal bipyramidal=

sp^3d hybridization

Ch. 6- 6 e- groups, octahedral=

sp^3d^2 hybridization

Ch. 4- mass to moles equation→

mass given/molar mass

Ch. 4- moles to mass →

given moles x molar mass

Ch. 4 atoms to moles →

given atoms/6.022 x 10^23

Ch. 4 moles to atoms →

given moles x 6.022 x 10^23

Ch. 4 mass to atoms →

given mass/molar mass x 6.022 x 10^23

Ch. 4 atoms to mass →

given atoms/6.022 x 10^23 x molar mass

Ch. 4 % mass=

mass of element/molar mass of compound x 100

Ch. 4 Steps to the empirical formula

Convert % to grams

Convert masses to moles

Divide all moles by smallest mole sum, round

Multiply all numbers of the mole ratio to make whole numbers

Ch. 4- if mole number ends with .5 →

multiply all mole ratios by 2

Ch. 4- if mole number ends with .33 or .67 →

multiply all mole ratios by 3

Ch 4.- if mole number ends with .25 or .75 →

multiply all mole ratios by 4

Ch. 4 - if mole number ends with .2, .4, .6, .8

multiply all more ratios by 5

Ch. 4- molecular formula =

mm compound/mm of empirical formula compound

what is the e-/ molecular geometry

tetrahedral/bent

sp=

2 e- groups

sp^2

3 e- groups

sp^3

4 e- groups

sp^3d

5 e-groups

sp^3d^2

6 e- groups