1. Matter and Elements
Chemistry 1405

2. Classification of Matter
Matter is anything that occupies space and has mass
We can classify matter based on its state and its composition
whether it’s solid, liquid, or gas
its basic components

3. States of Matter Solid – has a definite shape and definite volume.
Liquid – has an indefinite shape and a definite volume. A liquid takes the shape of its container.
Gas – has an indefinite shape and an indefinite volume. A gas assume the shape and volume of its container.

4. Matter
Physical property –characteristic of a substance that can be observed without changing the substance into another substance. E.g Color, odor, taste, size, physical state, boiling point, melting point density, Texture, Mass, volume, weight.
The appearance of a substance may change while a physical property is being determined, but the substance’s identity will not. For example, the melting point of a solid cannot be measured without melting the solid, changing it to liquid.
Physical properties – color, odor, taste, physical state, boiling point, melting point, sublimation point, deposition point, density.
Chemical property – reaction with air, oxygen, acid, base, decomposition.
Chemical properties are influenced by temperature and pressure.

5. Matter
Chemical property – a characteristic of a substance that describes the way the substance undergoes or resists change to form a new substance.
Chemical Properties describe the ability of a substance to form new substances either by reaction with other substances or by decomposition.

6. Properties Physical Chemical Color Odor Porosity Boiling point
Solubility
Melting point
Chemical
Reactivity
Flammability
Stability
Rusting
Reacts with air

7. Classify each of the following as a physical or chemical property
1. aluminum has a silvery color.
2. The mass of lead
3. Gold has a density of 19g/cm3
4. Magnesium burns brightly when ignited. 5. Milk turn sour.
6. water boils at 1000c
7. Iron and oxygen form rust.
Physical Chemical
Physical Physical
Physical Chemical
Chemical

8. Intensive and Extensive Property
Intensive property – independent of the amount of substance present.
Examples – Temperature, color, Melting point and density
Extensive property – depends on the amount of substance present.
Examples – mass, volume, length

9. Matter
Physical change – process in which a substance changes its physical appearance but not its chemical composition.
Examples:
Melting ice
Cloud formation
Making rock candy
Cutting into smaller pieces

10. Gas phase
Evaporation
Condensation
Sublimation
Deposition
Melting
Freezing
Solid phase
Liquid phase

11. Matter Others? Burning Food digestion Plant growth Healing of a wound
Chemical change – process in which a substance undergoes a change in chemical composition. A new substance is formed.
Burning
Food digestion
Plant growth
Healing of a wound
Rust
Fermentation
Others?

12. Chemical Reaction or Physical Change?
If the composition does not change, the change is physical.
If the composition does change, the change is chemical. It can be very difficult to recover the original material in a chemical change.

13. Classification of Matter by Composition
Matter whose composition does not change from one sample to another is called a pure substance
physical combination of two or more pure substances in which each substance retains its own chemical identity. mixture
Classification of Mixtures
Homogeneous mixtures are mixtures that have uniform composition throughout
Heterogeneous mixtures are mixtures that do not have uniform composition throughout

14. Types of Mixtures Heterogeneous Homogeneous
Two or more visibly distinct phases.
Each phase has different properties.
Examples?
Homogeneous
Only one visibly distinct phase.
The phase has the same properties throughout.
Examples?
Heterogeneous mixtures: rocks, soil, wood, salt/pepper, sand/water, oil/vinegar. If shaken is the oil/water mixture still heterogeneous? Yes – it is just emulsified. Milk is a heterogeneous mixture.
Homogeneous mixture – cool aide, salt water (but not necessarily sea water), older “silver” coins – 90% silver, 10% Cu.

15. Types of mixture
A homogeneous mixture has a constant composition throughout; it always has a single phase. Examples of homogeneous mixture
Sugar and water Mixture.
Milk
Motor oil and gasoline are homogeneous mixture of liquids.
Mixture of copper and Gold

16. Mixtures
A mixture is a combination of two or more pure substances in which each substance retains its individual chemical properties.
Mixtures can be separated by physical means.
Example of a mixture sand and water mixture, sand and iron fillings.

18. Pure Substance or Mixture
Elements are pure substances.
Elements are made from atoms.
Cannot be broken down into simpler substances by chemical or physical means.
Building blocks for all other types of matter..
Each has its own name,
symbol, and unique
characteristics.

19. Three Types of Elements
Metals :A metal is a good conductor of heat and electricity.
Nonmetals : A non metal is not a good conductor of electricity.
Metalloid: A metalloid has properties that are intermediate between those of metals and nonmetals

20. The periodic Table of Elements
The periodic table organizes the elements into a grid of horizontal rows called periods and vertical columns called groups or families.

21. ELEMENTS OF THE PERIODIC TABLE
Metals, Nonmetals, and Metalloids

22. = Alkali metals = Alkali earth metals = Noble gases = Halogens
= Lanthanides
= Actinides
= Transition metals
add pictures of elements from text
Tro: Chemistry: A Molecular Approach, 2/e

23. Symbol
Element Name Ag
Silver* Be
Beryllium Cr
Chromium Al
Aluminum Br
Bromine Cu
Copper* Ar
Argon C
Carbon F
Fluorine Au
Gold* Ca
Calcium Fe
Iron* B
Boron Cl
Chlorine H
Hydrogen Ba
Barium Co
Cobalt He
Helium

24. Symbol
Element Name Hg
Mercury* Na
Sodium* Pt
Platinum I
Iodine Ne
Neon S
Sulfur K
Potassium* Ni
Nickel Si
Silicon Li
Lithium O
Oxygen Sn
Tin* Mg
Magnesium P
Phosphorus U
Uranium N
Nitrogen Pb
Lead* Zn
Zinc
* Latin name

25. Pure Substance or Mixture
Compounds are also pure substances.
They are a chemical combination of two or more atoms.
Can be broken down into constituent atoms using chemical but not physical means.
Have a definite, constant elemental composition.
Rules exist for combining
atoms into compounds.

26. Chemical Formulas
Molecular Compounds – formula represents composition of molecules making up compounds.
Ionic Compounds – Formula represents ratio of ions in the compound since these are not considered molecules. A formula unit is used to describe the smallest ratio between ions. NaCl

27. Common Compounds Baking soda NaHCO3 Sodium carbonate
Epsom salt MgSO4 Magnesium sulfate
Clorox NaClO Sodium hypochlorite
Lime water Ca(OH)2 Calcium hydroxide in water
Vinegar CH3COOH Acetic acid
Table salt NaCl Sodium chloride
Chalk CaCO3 Calcium carbonate
Ethyl alcohol C2H5OH Ethanol
Ammonia NH3

28. Pure Substance or Mixture
Physical combination of two or more substance
Variable composition
Properties vary as composition varies
Components can be separated using physical means.
Pure Substance
Only one substance is present
Definite and constant composition.
Properties are always the same under a given set of conditions.
Cannot be separated by physical means.

29. Mixture or Pure Substance?
Crystalline sugar
Sugar water solution
Solid gold bullion
Steel
Milk

31. Pure Substances vs. Mixtures
Identify these as chemically and physically heterogeneous or homogeneous:
Glass of water at room temperature
Salad dressing
Glass of kool-aid.
Glass of ice water