Download - Matter Pure Substances Elements Compounds & Molecules Mixtures Homogeneous Solution Heterogeneous
Matter
Pure Substances
Elements
Compounds & Molecules
Mixtures
Homogeneous
Solution
Heterogeneous
Matter
Matter is anything that has MASS and takes up SPACE
Law of Conservation of Mass: Matter cannot be created or destroyed
Matter
Examples of Matter:• Water• Chex Mix• Plastic• Humans• Air
Examples that aren’t Matter:• Space• Light• Sound• Energy• Heat
The Atom: The unbreakable building blocks that make up all matter
Nucleus:Middle of the atom, made up of protons (+ charge) and neutrons (no charge)
Electrons ( - charge)
Physical Properties
All matter has physical and chemical properties
Physical Properties are properties that you can measure or see
Examples: mass, density, color, temperature, malleability and brittleness, phase (solid, liquid, gas)
Physical Changes
Physical changes change the physical properties but DO NOT change the matter into something else• Phase Changes• Changing Shape
Physical Changes are reversible
Chemical Properties
Chemical Properties are properties that allow the ability for a chemical change/reaction to occur
They can only be observed when matter goes through a chemical change, can’t know just by looking at itExamples: Flammability, Ability to react with specific materials
Chemical Changes
Chemical Changes: Any change that changes one substance into a different substance
Created by a chemical reaction
Chemical changes are very difficult or impossible to undo
Signs of a Chemical Change
Types of MatterMatter is separated into two major categories:
1) Pure substance cannot be separated into different kinds of matter by physical means and are made up of one single chemical throughout
2) Mixtures are made up of multiple substances
Most matter in the world around us are mixtures
Matter
Pure Substances
Elements
Compounds & Molecules
Mixtures
Homogeneous
Solution
Heterogeneous
Elements
Element: a substance that cannot be separated into simpler substances by chemical means• Each element is a unique type of atom• Atoms of the same element are all similar to
each other and different from atoms of any other element
• Elements are located on the periodic table
Periodic Table Layout
Organized into periods (rows) and groups (columns), elements separate from the table are part of Periods 6 and 7
Periodic Table
Element Symbol: 1 or 2 letters that represent the elementFirst letter is ALWAYS capitalized, second letter NEVER is
Atomic Number: Number of Protons
Atomic Mass
The atomic mass listed for an element on the periodic table is the mass of a single atom in atomic mass units (amu)
1 amu = 1.66 x 10-24 grams
Atomic mass units are not practical for experiments, our balances can’t measure a mass that small
Atomic MassTo turn amu into something more usable in lab we use a unit called the mole
1 mole = 6.02 x 1023 atomsThis is Avogadro’s Number
Atomic Mass = Number of grams in 1 mol
Calculating Moles using Atomic Mass
Use atomic mass as a conversion factor between moles and grams
How many moles are in a 10.0g sample of Carbon?
10.0 grams x 1 mole = 0.833 moles 12.01g
Try it on your own
You have 20 grams of Helium, how many moles do you have?
Calculating Mass from Moles
You have 5 moles of Nitrogen, how many grams do you have?
5 moles x 14.00 grams = 70 grams1 mole
Try it on your own
You have 2 moles of Lithium, how many grams do you have?
Matter
Pure Substances
Elements
Compounds & Molecules
Mixtures
Homogeneous
Solution
Heterogeneous
Review - Types of MatterMatter is separated into two major categories:
1) Pure substance cannot be separated into different kinds of matter by physical means and are made up of one single chemical throughout
2) Mixtures are made up of multiple substances
Most matter in the world around us are mixtures
Compounds and Molecules
Compounds and molecules are pure substances
They cannot be separated by physical means but can be separated by chemical means
Their physical and chemical properties come from the shape of the molecule, not from what they are made of
Compounds vs. Molecules
A molecule is ANY group of atoms chemically bonded together
Examples: H2 (Hydrogen Gas) CH4 (Methane)
N2 (Nitrogen Gas)
Compounds vs. Molecules
A compound is a substance containing DIFFERENT elements that are chemically bonded together.
Examples: H2O (Water)
C2H6O (Ethanol)
NaCl (Salt)Almost everything in this world is made of compounds!
Understanding Chemical Formulas
Chemical formulas are written using element symbols
Remember: Element symbols can have either 1 or 2 letters and ALWAYS start with a capital letter!
Chemical Formula PracticeHow many different elements are in each molecule?
NaCl KI
HCN KCl
MgO Xe
Subscripts
Subscripts are used to tell you how many copies of an element is in a molecule
H2 = 2 Hydrogen in one element
H2O = 2 Hydrogen, 1 Oxygen in one element
Practicing Reading Subscripts
H(CO3)2
How many H’s
How many C’s
How many O’s
H2SO4
How many H’s?
How many S’s?
How many O’s?
Molar Mass
Molar mass = Number of grams in one mole of the molecule
You need to add up the atomic mass of each element (multiplied by any subscripts) to get the total mass of the molecule
Practicing Molar Mass
Molar Mass of HCN
Mass of Hydrogen: 1.008Mass of Carbon: 12.01Mass of Nitrogen: 14.01
Molar Mass of HCN = 1.008 + 12.01 + 14.01 = 27.03 g/mol
Molar Mass of H2SO4
Mass of H: 1.008 x 2Mass of S: 32.07Mass of O: 16.00 x 4
Molar Mass of H2SO4 =
2.016 + 32.07 + 64.00 = 98.09 g/mol
Converting between grams and moles for molecules
Converting between grams, moles, and atoms is the same process for molecules as it is for individual elements
Instead of using atomic mass to convert between grams and moles you need to use the molar mass of the molecule
Molecule Conversion Example
You have 100 grams of Table Salt (NaCl), how many moles do you have?
100g NaCl x 1 mol NaCl = 1.71mol NaCl
58.44g NaCl
Molar Mass
Molar mass = Number of grams in one mole of the molecule
You need to add up the atomic mass of each element (multiplied by any subscripts) to get the total mass of the molecule
Percent (%) Composition
Remember from Lab 1C
% composition = mass of the part x 100
mass of the whole
We can find the Percent Composition of a molecule the same way
Percent Composition of Molecules
% comp = molar mass of element x 100
molar mass of molecule
Example: What percentage of the mass of H2SO4 comes from the Oxygen?
Mass of O: 16.00 x 4 = 64 g/molMass of H2SO4: 98.09 g/mol
% Oxygen: (64/98.09) x 100 = 65.2%
Percent Composition Example
Find the Percent Composition of both Copper and Chlorine in CuCl2
Molar Mass of Copper:Molar Mass of Chlorine:Molar Mass of Molecule:
% composition of Copper:
% composition of Chlorine:
Matter
Pure Substances
Elements
Compounds & Molecules
Mixtures
Homogeneous
Solution
Heterogeneous
Mixtures
Mixtures: Matter that contains more than one substance
Mixtures can be separated by physical means- sorting, filtering, heating, or cooling
Types of Mixtures
Homogeneous Mixtures looks the same throughoutHeterogeneous Mixtures look different throughout
Examples of MixturesDecide whether each mixture is a homogeneous mixture (HoM) or a heterogeneous mixture (HeM)
SoapChocolate Chip CookieGraniteGatoradeShampoo
Chex MixSandLemonadeGranola BarMilk
Matter
Pure Substances
Elements
Compounds & Molecules
Mixtures
Homogeneous
Solution
Heterogeneous
Solutions
Solutions are a specific type of homogeneous mixture where one substance (solute) gets dissolved in another substance (solvent)
The substance being dissolved (the solute) completely breaks down and gets absorbed by the solvent:
Examples: Salt Water, Pop, lemonade