1. Topic 1.1 Matter & Change
EI: physical and chemical properties depend on the ways in which different atoms combine.
NOS: Making quantitative measurements with replicates to ensure reliability – definite and multiple proportions (3.1)

2. What is Matter? What is Matter?
Anything that takes up space and has mass.
Made up of particles (atoms, molecules, ions)
Particles are in constant motion

3. Distance between particles Arrangement of particles
A 2. States of Matter
State
Shape
Volume
Distance between particles
Arrangement of particles
Solid (S)
Fixed shape
Fixed volume
Close together
regular
Liquid (l)
No fixed shape
Fixed volume
Close, but farther than solids
random
Gas or Vapor (g)
No fixed shape
Not fixed
Far apart
random

4. Switching between states
Solid  melting  Liquid
Liquid  freezing  Solid
Liquid  evaporating (boiling)  Gas
Gas  condensing  Liquid

5. Switching between states
Solid  sublimation  Gas
Gas  deposition  Solid
Heat is required from solid to liquid to gas
Heat is removed from gas to liquid to solid

6. Switching between States

7. U1: Properties of Matter
Physical property
A characteristic of a substance that can be measured or observed without changing the substance’s composition
Chemical property
The ability of a substance to undergo a chemical reaction to form new substances

8. Examples of Physical Properties Examples of Chemical Properties
U1. Properties of Matter
Examples of
Physical Properties
Color
Solubility (Dissolving)
Odor
Hardness
Density
Melting Point
Boiling Point
State of matter
Thermal capacity
Mass
Examples of
Chemical Properties
Reactivity with oxygen
Reactivity with acids
Reactivity with bases
Reactivity with other elements
Sodium and Chlorine Reaction

9. U1. Properties of Matter
Sodium is a silver metal at room conditions; combines with chlorine to make table salt; reacts with water to form hydrogen; has a density of 0.93 g/cm3; oxidizes rapidly in air, melts at 97.8oC.
Using the above description, list the physical properties of sodium
Using the above description, list the chemical properties of sodium

10. U1. Properties of Matter
Sodium is a silver metal at room conditions; combines with chlorine to make table salt; reacts with water to form hydrogen; has a density of 0.93 g/cm3; oxidizes rapidly in air, melts at 97.8oC.
Using the above description, list the physical properties of sodium
Using the above description, list the chemical properties of sodium

11. U1. Changes of Matter Physical change
An alteration of matter that does not change the chemical composition of the material.

12. U1. Changes of Matter . Chemical change
Results in a change in the chemical composition of the substance(s). This is called a reaction.

13. U1. Changes of Matter Examples of Physical Changes Examples of
Freezing or melting
Boiling or condensing
Cutting
Grinding
Bending
Blending
Dissolving
Examples of
Chemical Changes
Combustion (burning)
Reacts with an acid
Reacts with a base
Rusting
Oxidizing
Decomposing
Digesting

14. U1. Changes of Matter Copy the statement on your paper and write P for physical or C for chemical
Bending of a piece of wire
Burning of coal
Cooking a steak
Cutting grass
Sodium reacts with water
6. Iron rusts
7. Silicon is insoluble in water
8. Ice melts
9. Neon boils at -2460C
10. Nitric Acid reacts with Copper

15. U2. Distinguishing Compounds and Mixtures
Elements are composed of just one type of atom. They cannot be separated into simpler substances using chemical means.
Stop Here do to the physical/chemical lab 2014

16. U2. Distinguishing Compounds and Mixtures
Compounds are substances composed of two or more different kinds of atoms that have combined chemically. They can be separated by chemical means.
Stop Here do to the physical/chemical lab 2014

17. U2. Distinguishing Compounds and Mixtures
Mixtures are a physical blend of two or more substances. They can be separated by physical means.
Stop Here do to the physical/chemical lab 2014

18. U2. Distinguish compounds and mixtures
Elements
Represented by a chemical symbol (see Periodic Table)
Gold (Au), Iron (Fe), Oxygen (O or O2)
Start here after physical/chemical change lab

19. U2. Distinguish compounds and mixtures
A fixed ratio of elements, shown using element symbols and a number

20. U2. Distinguish compounds and mixtures
Examples:
Water, H2O, contains 2 atoms of hydrogen (H) and one atom of oxygen(O).
Salt, NaCl, contains one atom of sodium (Na) for each atom of chlorine (Cl).

21. U3. Mixtures Mixtures: composition is not fixed
Homogeneous mixture- has uniform composition and properties, also called solutions.
Ex: pure air, pure water, syrup

22. U3. Mixtures
Mixtures:
Heterogeneous mixture – non-uniform composition, properties are not the same, able to see the separate components
Ex: soup, concrete, granite

23. Ways to separate mixtures:
U3. Mixtures
Ways to separate mixtures:
Heterogeneous: sieving, tweezers, skimming
Homogeneous: distillation, ion exchange, reverse osmosis, evaporation

24. Distinguish between elements, compounds, and mixtures Copy the item and indicate if it is an element, compound or mixture
6. Silver
7. Orange juice
8. Neon
9. Sugar (C6H12O6)
10. Lake water
Blood
Hydrogen
Brass (copper and zinc)
Ice (H2O)
Motor oil
Practice Problems: pg. 40
14-18

25. A& S. 1: Chemical Reactions
In a chemical reaction, one or more substances change into new substances by rearranging the atoms
Reactants  Products

26. A& S. 1: Chemical Reactions
Reactants  Products
Reactants: the substances that are combined together
Products: the substances that are formed after the reactants are combined together.

27. A& S. 1: Chemical Reactions
Chemical Reaction Example:
Reactants  Products
Copper+ nitric acid copper(II) nitrate+ nitrogen dioxide+water
Cu + HNO3  Cu(NO3)2 + NO2 + H2O

28. A& S. 1: Chemical Reactions
Reactants  Products
Copper+ nitric acid copper(II) nitrate+ nitrogen dioxide+water
Cu + HNO3  Cu(NO3)2 + NO2 + H2O

29. A&S 1. Chemical Reactions
A chemical reaction has occurred if:
Heat is absorbed or given off (change in temperature)
Change in color or odor
Production of a gas or solid
Not easily reversible

30. A&S 1. Chemical Reactions
Law of Conservation of Mass
During any chemical reaction, mass is neither created nor destroyed, it is conserved.
The mass of the products will always equal the mass of the reactants.
The mass of each element is also unchanged.

31. A&S 1. Chemical Reactions
Law of Conservation of Mass
In a reaction where hydrogen reacted with oxygen to produce water, if 4.5 g of hydrogen and 34 g of oxygen were used, how many grams of water were produced?
Hydrogen + oxygen = water
= 38.5 g water