Chemistry Common Knowledge Flashcards
Shows exact # of Atoms of each Element
Molecular Formula
Shows which elements are present & the simplest whole number ratio of their atoms
Empirical Formula
Shows exact # of Atoms of Each Element
Molecular Fórmula
Properties of metals & non-metals
Metalloids
Constant composition, cannot be separated into smaller substances by physical process
Pure Substance
Transforms a sample of matter w/o altering chemical identities of any substance in the sample (ex- changing a liquid to solid)
Physical Process
Pure substance (cannot be broken down)
Element
Gold, silver, nitrogen, oxygen, sulfur
Pure substances (natural/uncombined)
2 or more elements that can only be separated by a chemical reaction
Compound
2 + substances of matter - each retains its chemical identity (can be separated by physical process)
Mixture
Uniform mixtures / Solutions
Homogeneous
Not uniform / not clear / not transparent
Heterogeneous
Quantity of matter
Mass
Everything that has mass and takes up space
Matter
1st elements formed in the universe
Hydrogen & Helium
Study of the composition, structure, & properties of matter, and its changes
Chemistry
A concise statement of a relationship between phenomena that is always the same under the same conditions
Law
Mass X Acceleration =
Force
Unifying principle- explains a body of facts and/or those laws that are based on them
Theory
A tentative explanation for a set of observations
Hypothesis
Compounds always contain the same elements in the same composition
Law of Constant Composition
Positive charge
Cation
Negative charge
Anion
Cannot be separated into simpler substances by chemical means
Element
Does not alter the composition or identity of a substance
Physical change
Ice melting
Sugar dissolving in water
Alters the composition or identity of the substances involved
Chemical change
Of a material that depends upon how much matter is being considered (mass, length, volume)
Extensive Property
Does not depend upon how much matter is being considered (density, temperature, color)
Intensive property
Length
Meter (m)
Mass
Kilogram kg
Time
Second S
Electrical Current
Ampere A
Temperature
Kelvin K
Amount of substance
Mole (mol)
Luminous Intensity
Candela (cd)
Force gravity exerts on an object
Weight
Occupies space and has mass
Matter
Quantity of matter
Mass kg / gram
Force gravity exerts on an object
Weight
Shows the exact number of atoms of each element H2O2 N2H4
Molecular Fórmula
Shows which elements are present and the simplest whole number ratio of their atoms
Empirical Formula
Atomic mass - Atomic number =
of neutrons
Polyatomic Ions
Ions made up of many atoms (2 or more)
The Mole
Avogadro’s #
6.02 x 10^23 things in 1 Mole
The Mole
Avogadro’s #
6.02 x 10^23 things in 1 Mole
What does 1 mole = ?
6.02 x 10^23
Avogadro’s Number
Combines with
Addition
The Sum
Addition
Increases By
Addition
Plus
Addition
The Total of
Addition
And
Addition
The difference of
Subtraction
Minus
Subtraction
Decreases by
Subtraction
Less than
Subtraction
Reduced by
Subtraction
The product of
Multiplication
Times
Multiplication
Of
Multiplication
The ratio of
Division
The quotient of
Division
= and
—> in a chemical equation
Form
Produce
Create
Yield
Result
4 States in a Chemical Equation
Aqueous (aq)
Liquid (l)
Solid (s)
Gas (g)
Aqueous
Dissolved
Dissociated
Ionized
Aqueous
Na+(aq)
Aqueous solution of Salt
Liquid (l)
H2O
Can also be a solid or gas so never assume water is a liquid
Solid (s)
Precipitate
Metal
Gas (g)
Vapor
Gaseous
Diatomic molecules
Elements that exist in pairs
Diatomic Molecules H2, O2, N2, F2, Cl2, Br2, I2
Reactants
Reacts with or
Combines with
Products
Forms
Yields
Creates
Results in
Converts into
Produces
Combines with
Reactant
Yields
Products
Combines with
Reactants
Forms
Products
Converts into
Products
Forms
Products
Left side of arrow ——-> Right side of arrow
Reactants ———> Products
Decomposes
Decomposition Reaction
AB —->. A + B
Ex. CO2 —-> C + O2
A compound is broken down to multiple products
Rust means what type of reaction ?
Single Replacement Reaction
A + BC ——> AB + C
Ex.
Mg + 2 HCl ——> MgCl2 + H2
1 single element Mg, replaces another element (H) in a compound to form a new compound + an element MgCl2 + H2
Combustion Reaction
Combusts or Burns
CxHy + O2 —-> CO2 + H2O
The only thing that changes is CxHy reactant
CxHyO2 + O2 —-> CO2 + H2O
The +O2 js always your reactant and the product is always Carbon Dioxide & Water
Exs.
CH4 + 2O2 —-> CO2 + 2H2O
CH4O + O2 —-> CO2 + 2H2O
Keyword Precipitate
Precipitation Reaction
Looks like :
Reactants AgNO3(aq) + KCl(aq) area aqueous
——> AgCl(s) + KNO3(aq)
——> and 1 solid is formed
The solid is your Precipitate AgCl(s)
Translate word problem:
Gaseous propane C3H8, burns into oxygen gas to produce carbon dioxide gas and liquid water
C3H8 is a gas / Burns=combustion reaction
ends with CO2+H2O
C3H8(g) + O2(g)
Produce ——-> tells us our products are Carbon Dioxide (g) & water (l)
C3H8(g) + O2(g) —> CO2(g) + H2O(l)
Our balanced chemical equation looks like :
C3H8(g) + 5 O2(g) —> 3 CO2(g) + 4 H2O(l)
Mercury (II) oxide in its metal state decomposes to produce liquid mercury and oxygen
Decomposition Reaction AB —> A+B
Mercury (II) oxide solid state
Produce = —->
HgO2(s) ——> Hg(l) + O2(g)
Oxygen is a diatomic molecule that exists in pairs and it is a gas
Molarity OF Dilutions
How to use and translate : OF
Ex. O.2 L of 15.0 M
Volume. Molarity or Concentration (M)
(mL or L). Of a Solution
Dilutions formula for
Molarity (M) —> M1V1 = M2V2
Molarity1Volume1=Molarity2Volume2
Concentration (M)—-> C1V1 = C2V2
Still measured in molatity
