5923781
Description
Chemical
Formula &
Equation
- Chemical Reaction
- Avogrado's
Constant
- Number of atoms in 12g of carbon-12 atom
- 6.002x10^23
- 6.002x10^23
- Number of atoms in 12g of carbon-12 atom
- Moles
- Number of atoms and molecules
- Number of moles(mol)=mass(g)/molar mass(g mol^-1)
Annotations:
- Number of moles(mol)=mass(g)/molar mass(g mol^-1)
- Number of moles(mol)=mass(g)/molar mass(g mol^-1)
- Number of atoms and molecules
- Molar
Volume
- Standard temperature and volume:22.4L
mol^-1
- Volume occupied by 1 mol of gas
- Volume occupied by 1 mol of gas
- Standard temperature and volume:22.4L
mol^-1
- Chemical formulaes
- Molecular formula
- Chemical formula which shows the
actual number of atoms in an element
- n(empirical
formula)
- n(empirical
formula)
- Chemical formula which shows the
actual number of atoms in an element
- Empirical formula
- Chemical formula which shows the
simplest ratio of atoms of an element
- Steps
- 1)Determine the mass or percentage(by 100g)
of elements in the compound
Annotations:
- 1)Determine the mass or percentage(by 100 g) of elements in the compound 2)Divide the mass/percentage of elements with respective relative atomic mass 3)Divide by the smallest number to obtain the ratio 4)Write the empirical formula from the ratio of the elements
- 2)Divide the mass or percentage of elements
with the respective relative atomic mass
- 3)Divide with the smallest
number to obtain the ratio
- 4)Write the empirical formula
from the ratio of the elements
- 4)Write the empirical formula
from the ratio of the elements
- 3)Divide with the smallest
number to obtain the ratio
- 1)Determine the mass or percentage(by 100g)
of elements in the compound
- Steps
- Chemical formula which shows the
simplest ratio of atoms of an element
- Molecular formula
- Avogrado's
Constant
- Concentration
of Solutions
- A solution is a
homogenous
mixture of two or
more substances
- solvent + solute(s)
- solvent + solute(s)
- Expression
- Mole
Fraction (X)
- Xa = moles of a /
sum of moles of
all components
- Xa = moles of a /
sum of moles of
all components
- Percentage by
mass and volume
- %w/w = (Mass of X /
Mass of sample) x100%
- %w/V = (mass of X
(g) / Volume) x100%
- %v/v = (Volume of X /
Volume of Sample) x100%
- %w/w = (Mass of X /
Mass of sample) x100%
- Molality
- Molality,m = moles of solute (mol)
/ mass of solvent (kg)
- Molality,m = moles of solute (mol)
/ mass of solvent (kg)
- Molarity
- Molarity = moles of solute
/ liters of solution
- Units
- mol L^-1
- mol dm^-3
- M
- mol L^-1
- Molarity = moles of solute
/ liters of solution
- Mole
Fraction (X)
- A solution is a
homogenous
mixture of two or
more substances
- Dilution
- procedure for preparing a less
concentrated solution from a
more concentrated solution
- M1V1 = M2V2
- procedure for preparing a less
concentrated solution from a
more concentrated solution
- neutralization
reaction
- acid + base ---> salt + water
- acid + base ---> salt + water
- Oxidation
Number
- Number that is
assigned to an
atom in a
substance
- Indicates if electron
are lose or gain
- Positive
- Atom loses
electron
- eg. Ca2+ ,
atom lose 2
electron
- Atom loses
electron
- Zero
- Atoms neither
gains nor lose
electrons
- Atoms neither
gains nor lose
electrons
- Negative
- Atoms
gain
electron
- eg. O2- ,
atom gain
2 electrons
- Atoms
gain
electron
- Positive
- Rules
- Pure
Elemental
Form
- Atom that is not
combined with
other element
- Oxidation Number = 0
- eg : Ag, He, Cu
- Atom that is not
combined with
other element
- Ions
- Atom with charge due to
the gain or lose of electrons
- Oxidation Number = charge for ions
- eg: H+
oxidation
number = +1
- Atom with charge due to
the gain or lose of electrons
- Neutral
Compound
- Sum of oxidation number =
0
- eg. HCl, NaOH
- Sum of oxidation number =
0
- Hydrogen
- 2 Possible oxidation number
- +1
- -1
- +1
- +1
- Bonded to non-metal
- eg: HCl - H+
- Bonded to non-metal
- -1
- Bonded to metal
- eg: NaH - H-
- Bonded to metal
- 2 Possible oxidation number
- Pure
Elemental
Form
- Calculation
- Calculate the oxidation
number of the element in
neutral compound
- eg. Hydrogen Fluoride
- H = +1
F = ?
- -1 + F = 0
- F = -1
- Therefore, the oxidation
number of fluorine is -1
- Therefore, the oxidation
number of fluorine is -1
- F = -1
- -1 + F = 0
- H = +1
F = ?
- Calculate the oxidation
number of the element in
neutral compound
- Number that is
assigned to an
atom in a
substance
- Limiting Reagent
- Reaction
- The reaction that stops once the limiting reagent is gone
( no matter how much the excess is present)
- The reaction that stops once the limiting reagent is gone
( no matter how much the excess is present)
- Limiting Reagent
- Substance that are totally consumed
when the chemical reaction is complete
- Substance that are totally consumed
when the chemical reaction is complete
- Excess Reagent
- The reactant presents in quantities greater than
necessary to react with the quantity of the
limiting reagent
- The reactant presents in quantities greater than
necessary to react with the quantity of the
limiting reagent
- Percentage Yield %
- Theoretical yield
- The amount of
product that would
result if all the limiting
reagent reacted
- The amount of
product that would
result if all the limiting
reagent reacted
- Actual yield
- The amount of product
actually obtained from
reaction
- The amount of product
actually obtained from
reaction
- % yield
- Actual Yield / Theoretical Yield x 100
- Actual Yield / Theoretical Yield x 100
- Theoretical yield
- Reaction
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