Unit 0 Exam 1 Review
Nomenclature: Covalent compounds
Covalent compounds
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Between a nonmetal and a nonmetal
Know the elements that are in covalent
compounds:
H, C, N, O, F
Si, P, S, Cl
Br
I
Know these 3 famous polyanions:
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SO4-2≡sulfate
NO3-≡nitrate
PO4-3≡phosphate
Know how to name neutral compounds.
AXBX
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A= say the name of the element with a prefix, if
the number is greater than one.
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B= Add prefix and say the name of the
element with a suffix of “-ide”
Prefixes:
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2≡di
3≡tri
4≡tetra
5≡pent
6≡hex
Nomenclature of Ionic compounds
Salts involve elements from opposite sides of the main group (AxBy)
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A = cation:written as the element’s name
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B = anion:written as the element’s name with the suffix “ide”
x= # of cations
y= # of anions
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Group I, II, III are cations
Like Na, Ca and Al
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Group V, VI, VII are anions
Like N, O, and Cl
Transfer the charges when writing the ionic formula
*if they are the same charge drop the subscripts*
Nomenclature of transition metals
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When writing the name of the compound
include the charge of the transitional metal
as a roman numeral
When writing the formula transfer the
charges of each element.
Example:
Iron (Ⅲ) oxide
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Means iron has a +3 charge
Fe3+ and O2Fe2O3
Organic parent compounds
Number
of
Carbons
prefix
Number of bonds
1
meth-
2
eth-
3
prop-
4
but-
5
pent-
6
hex-
7
hept
8
oct
Suffix
Single bond
-ane
Double bond
-ene
Triple bond
-yne
Atom structure
Proton mass is 1 = amu ≈ 1 gram/mole. Charge is +1
Neutron mass is 1 amu ≈1 grams/mole. Charge is neutral
Electron mass is 1/2000 of a g/mole. Charge is negative
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Protons = atomic number and is what determines the type of element. It Increases by 1 from 1 for H to 118 for Og on
the periodic table
Neutrons = determines the isotope of an element
Electrons = balances charge of proton, also the key particle that creates chemical reactions to make different kinds of matter.
MKS units
Length
Meters (m)
Time
Seconds (s)
Mass
Kilogram (kg)
Energy
Joules (J)
Temperature
Kelvin (K)
Quantity of matter
Mole (mol)
Electric current
Ampere (A)
Scientific notation math
Conversion of mks units
1min=60𝑠
212𝑔𝑟𝑎𝑚𝑠=0.212𝑘𝑔
550𝑐𝑚=5.5𝑚
Approximations
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a mathematical quantity that is close in value to but not the same as a desired quantity.
Functional relationships
Functions
Equations
Graphs
Explanation
Direct Proportional
(Linear)
y=mx+b
As x increases y
increases at the same
rate. x ∝ y
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A = abc
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A ∝C
Inverse Proportional
(Reciprocal)
y=1/x
As x increases, y
decreases. x∝ 1/y
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PV=nRT
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As P↑, V will↓
Quadratic or
Parabola
y=x^2
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Rate = k[A]^2
As [A] increases
rate increases as a
rough square
Functional relationships
Functions
Inverse square
Equations
y=1/x^2
Graphs
Explanation
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ν=
R(1/n1^2−1/n2^2)
As n↑, ν decreases
as a rough inverse
square
Logarithmic
y =ln(x)
Logarithmic functions
are the inverses of
exponential functions.
Exponential
y = 2^x
An example of an exponential
function is the growth of bacteria.
Some bacteria double every
hour. If you start with 1
bacterium and it doubles every
hour, you will have 2x bacteria
after x hours. This can be written
as f(x) = 2x
Periodic table
Periodic table review
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Columns = groups = families. These elements share the same characteristics.
Rows = periods
Extracting information from the periodic table
Atomic number = # of protons
Atomic mass
*Electron # = Protons, if the charge is
neutral
*Neutron #= mass number-proton
number
Valence electrons
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The group number tells tells you the number of valence electrons.
Example:
Oxygen is in group 16.
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Group 16 has 6 valence electrons
Types of reactions