1. Unit1: Matter Review

2. General Properties of Matter
Matter is anything that has mass and volume
Everything is made of matter

3. General Properties of matter
Mass, weight, volume, and density
Properties are used to identify a substance

4. States of matter Four states of matter: solid, liquid, gas, and plasma
solids have a definite shape and volume
Solids are tightly packed and the particles vibrate

5. Physical Properties of Matter
Hardness – a measure of the resistance of a solid to being scratched or dented.
Malleability – When a solid can be hammered into sheets or bent into shapes.
Ductility – solid can be pulled into wires.
Crystal form – when a definite structure of blocks or cubes in a regular pattern form.

6. Physical Properties of Matter
Solubility – the ability of a substance to dissolve in a solvent.
Viscosity – refers to how easily a liquid flows.
Density – the amount of matter per unit volume of that matter. Usually expressed in grams per cubic centimeter (g/cm3).

7. Chemical Properties
A chemical property is a behavior of a substance when it interacts with another substance. This usually forms a new substance.
Combustibility – describes the ability of a substance to react with oxygen to produce carbon dioxide, water and energy. If a substance is combustible or flammable, it will burn when exposed to a flame.

8. Physical Change
In a physical change, the substance involved remains the same substance.
Changes of state – melting, boiling, freezing, condensation, sublimation – are all physical changes.
Dissolving is also a physical change.
Most physical changes are easy to reverse.

9. Chemical Change
In a chemical change, the original substance is changed into one or more different substances that have different properties.
Chemical changes always involve the production of new substances.
Chemical changes are difficult to reverse.
Examples include burning, cooking and rusting.

10. How can you tell if a change is chemical or physical?
There are many signs that can tell us. Consider several clues before coming to a conclusion.
A new color appears
Heat or light is given off
Bubbles of gas are formed
A solid material (called a precipitate) forms in a liquid.
The change is difficult to reverse.

11. Chapter 2

12. The Particle Theory of Matter
All matter is made up of tiny particles.
All particles of one substance are the same. Different substances are made up of different particles.
The particles are always moving. The more energy the particles have, the faster they move.
There are attractive forces between the particles. These forces are stronger when the particles are closer together.

13. As well as classifying matter as solids, liquids, and gasses, we can classify matter as either a mixture or a pure substance.
A pure substance is made from only one type of particle. These specific particle types give the substance its physical characteristics such as odor, color, hardness.
A mixture contains two or more pure substances. (See Fig. 1 pg. 45)

14. A homogeneous mixture has two substances where the particles are blended completely. To the eye, the mixture appears to be pure substance.
When the particles stay intermixed and don’t settle into layers we call the homogeneous mixture a solution.

15. A heterogeneous mixture has large clumps of particles that don’t fully separate and get intermixed with the other substance.
Examples of heterogeneous mixtures are salad dressing, oil and water, pizza, etc.

16. Elements and Compounds
Elements are pure substances that cannot be broken down into simpler substances.
Compounds are pure substances that contain 2 or more elements in a fixed proportion. They are formed when elements combine together in chemical reactions.

17. What makes up an atom?
Three types of particles make up an atom; these are called subatomic particles.
Protons – positive charge, found in the nucleus.
Neutrons – no charge, found in the nucleus.
Electrons – negative charge, found orbiting the nucleus.

18. C Cu Chemical Symbols Carbon Copper
All elements have their own unique symbol.
It can consist of a single capital letter, or a capital letter and one or two lower case letters. C
Carbon Cu
Copper

19. Chemical Formulas
When atoms of different elements combine, they form compounds.
A chemical formula is the combination of symbols that represents a particular compound. (Table 2 pg. 59).
If there is more than one atom of the element in a compound, the symbol is followed by a number (called a subscript).
Eg. H2O = Water (2 atoms of Hydrogen and 1 atom of oxygen)

20. How can we determine the charge of an ion?
For some of the elements it is very easy. Elements in groups 1, 2, 13, 14, 15, 16, & 17 will lose or gain electrons so they have the same # as the nearest Noble Gas (group 18).
The transition metals (groups 3- 12) cannot have their charges predicted in this way due to many of them having isotopes. Their charges must be predicted in other ways.

21. Rules For Combining Elements
Rule 1: Metals combine with non metals in many compounds.
Rule 2: Write the name of the metal first and the non metal second.
Rule 3: Change the ending of the non metal to “ide.”
Rule 4: Each atom has its own combining capacity.
Rule 5: Atoms combine so that each can fill its own combining capacity.

22. When combining 2 ions, you need to create a net charge of zero.
Eg. Ca2+ + Cl CaCl2 (2 positives, 2 negatives = 0 charge)
If you do not know the combining capacity of the element, you can use your knowledge of ions. The charge of the ion is it’s combining capacity.
Use the following method to then make the compound

23. Ca2+ + O2- Mg2+ + Cl- Ca2O2 MgCl2 Crossing Over Method
(2’s cancel out) CaO = Calcium Oxide
Mg2+ + Cl-
= Magnesium Chloride
Ca2O2
MgCl2

24. Ch. 3

25. Atomic Models: Dalton
All matter is made of atoms, which are particles that are too small to see.
Each element has it’s own kind of atom with it’s own particular mass
Compounds are created when atoms of different elements link to form molecules.
Atoms cannot be created or destroyed or subdivided in chemical changes.

26. Atomic Models: J.J. Thompson
The atoms are neutral… How?
+ charges must be present to balance - charges
+ & - lumped in a cluster he said looked like “plum pudding”

27. Rutherford’s Atomic Model
Rutherford developed a new model for the atom.
An atom has a tiny, dense positive core called the nucleus (which deflected the alpha particles and contains protons.)
The nucleus is surrounded mostly by empty space, containing rapidly moving negative electrons (through which alpha particles pass unhindered.)

28. Atomic Models: Bohr
Niels Bohr proposed a “planetary” model of the atom.
Electrons are found in specific energy levels called orbits
Like planets around the sun

29. Atomic Models: Bohr
Each electron in an orbit has a definite amount of energy.
The further the electron is from the nucleus, the more energy it has.
Electrons do not exist between the orbits but can move from on orbit to another.
The order of filling of electrons in the first three orbits is 2, 8, 8.
Electrons are more stable when they are at lower energy, closer to the nucleus.

30. What’s in a square?
Different periodic tables can include various bits of information, but usually:
atomic number
symbol
atomic mass

31. Key to the Periodic Table
Elements are organized on the table according to their atomic number, usually found near the top of the square.
The atomic number refers to how many protons or electrons an atom of that element has.
For instance, hydrogen has 1 proton, so it’s atomic number is 1.
The atomic number is unique to that element. No two elements have the same atomic number.

32. Bohr Diagrams
Bohr’s model was readily accepted by scientists and they began drawing models of the atom using his theory.

33. Bohr-Rutherford Diagrams
This diagram is a combination of Rutherford's nuclear model and Bohr’s planetary model.
It summarizes all of the sub atomic particles in the atom

34. Chlorine
17 p+
18 n0

35. Isotopes
An isotope is any two or more forms of an element, each having the same number of protons, but a different number of neutrons.
Isotopes of the same element have the same chemical and physical properties.
Some isotopes are unstable, or radioactive, which means that the nucleus has a tendency to break apart and eject very high energy particles into its surroundings.
Atoms that have unstable nuclei are called radioisotopes.

36. Ch. 4

37. A Family is also called a Group.

38. based on their atomic numbers.

39. Groups or Families Periods
Each horizontal row of elements is called a period.
The elements in a period are not alike in properties.
In fact, the properties change greatly across even given row.
The first element in a period is always an extremely active solid. The last element in a period, is always an inactive gas.
The period tells us how many orbitals the element has.
Columns of elements are called groups or families.
Elements in each family have similar but not identical properties.
For example, lithium (Li), sodium (Na), potassium (K), and other members of family IA are all soft, white, shiny metals.
All elements in a family have the same number of electrons in their outer orbital.

40. Noble Gases
Noble Gases are colorless gases that are extremely un-reactive.
One important property of the noble gases is their inactivity. They are inactive because their outermost energy level is full.
Because they do not readily combine with other elements to form compounds, the noble gases are called inert.
The family of noble gases includes helium, neon, argon, krypton, xenon, and radon.
All the noble gases are found in small amounts in the earth's atmosphere.

41. Alkali Metals
The alkali metals (group 1A) are located in the far left column of the periodic table.
These metals are highly reactive and readily form compounds with other elements. Most commonly H, O, Cl, F, Br, I.
The reactivity of alkali metals is explained by their structure. These metals have only one electron in their outer orbital. They will readily lose this electron to become a stable atom.

42. Halogens
Group VII A
Include F, Cl, Br, I, At
Next to the noble gases
These are the most reactive non metals. They almost always appear naturally as compounds (Cl2, Br2 , etc.)
They make very useful compounds such as iodized table salt, chlorine in drinking water, sodium fluoride in toothpaste, etc.
The reactivity of halogens is explained by their structure. These non metals need only 1 electron to fill their outer orbital. They will readily gain this electron to become a stable atom.

43. A Group of One Hydrogen is a unique element.
It has only 1 electron. Therefore it has only one orbital (How many electrons can this orbital hold?)
It can react as both a metal and a non metal. It can either lose or gain 1 electron to become a stable atom.
Most of the Earth’s hydrogen exists in compounds due to it’s high reactivity.