1. Chemistry Review

2. All Matter in the universe is composed of…

3. ATOMS https://www.youtube.com/wa tch?v=joOYgeqMJwU https://www.youtube.com/wa tch?v=joOYgeqMJwU

4. ATOMS Elements are composed of only one type of atom Contain a nucleus which contain protons and neutrons

5. The force that hold two atoms together is a chemical bond. Two or more atoms that are bonded together form a molecule. Some are made up of only one type of atom but most are made up of two or more different types of atoms bonded together.

6. Electrons Negatively charged Orbit around the center of the atoms in orbits/shells called an electronic cloud The farther from the center, the _______ energy it has Gain and lose energy by moving between energy levels

7. In the nucleus of an atom PROTONS: Positively charged and have a mass of 1 The number of protons in an atoms nucleus determines what element it is The amount of positive charge on a proton is equal to the amount of negative charge on an electron NEUTRONS: Have no charge Mass of 1

8. Particle NameLocationChargeMass ElectronOrbitals~0 ProtonNucleus+11 NeutronNucleusNo Charge1

9. Atomic Number Every atom of the same element has the same number of protons It is the number of protons an element has which determines what element it is.

10. Mass Number = the total mass of an atom It is the same as the number of protons & neutrons of the element. One can calculate the number of neutrons an atom has by subtracting the atomic number (# protons) from the mass number. Mass number CAN change without changing the identity of the element Mass number CAN change without changing the identity of the element

12. Isotopes Not all atoms of the same element have the same number of neutrons Atoms of the same element that have different number of neutrons are called isotopes

13. Finding #’s Number of Protons = Atomic Number Number of Electrons = Number of Protons = Atomic Number Number of Neutrons = Mass Number - Atomic Number

15. Periodic Table Notation: Chemical elements are represented on the periodic table using the following format. The letter is an abbreviation of Element Name Atomic Number Mass number.

16. Structure Vertical columns are called groups or families Numbered 1-18 Elements in each group have similar properties Different elements with the same number of electrons in their outer energy level have similar chemical properties Use a dot diagram to represent electrons in the outer energy level

17. Dot Diagram

18. Groups #17 “Halogens” Group #18 “Noble Gases”

19. Structure Horizontal rows are called periods Look at the step line All elements to the left except hydrogen are metals The elements to the right of the line are classified as nonmentals Elements right next to the line are metalloids because they have properties of both metals and non mentals http://ritter.tea.state.tx.us/student.assessment/resourc es/online/2009/taks_g11_science/images/chart2.gif http://ritter.tea.state.tx.us/student.assessment/resourc es/online/2009/taks_g11_science/images/chart2.gif

20. Interactions of matter: Atoms interact through the process of chemical bonding. Process is determined by the number of electrons found in the outermost energy level of an atom. Involves the transfer & sharing of electrons between atoms.

21. Matter has a variety of characteristics or properties that can differ. They fall into 2 different groups used to identify, describe and classify matter: 1.Physical 2.Chemical

22. A single kind of matter that has distinct physical and chemical properties is called a substance.

23. A physical property can be observed without changing the substance into something else. OdorTasteHardnessTextureColor Temperature at which a solid melts or liquid boils Whether its solid, liquid or gas Physical Properties

24. A compound is a substance made of two or more elements chemically combined in a set ratio or proportion. Examples: Carbon Dioxide gas is a compound made up of Carbon and Oxygen. Water is a compound made up of oxygen and hydrogen.

25. When elements are combined to make a compound, the new substance has properties different from those of the original elements. Example: table sugar is made up of 3 elements- Carbon, Oxygen and Hydrogen. Carbon=found in charcoal Oxygen/hydrogen=colorless gases Do sugar crystals resemble them?

26. Most matter occurs in mixtures. A mixture is made from two or more substances (elements or compounds) that are in the same place but are NOT chemically combined.

27. Mixtures differ from compounds in 2 ways: 1.The substances in a mixture keep their individual properties. 2.The parts of a mixture are not necessarily present in set ratios. Example: soil has particles of sand, tiny bits of clay, and pieces of decaying plants. If you were to grab 2 handfuls of soil would they be made up of the same amount of clay, sand, and decaying plant matter?

28. Which is a mixture and which is a compound? Chex mix Table salt Water Muddy water Carbon dioxide Checkpoint

29. A chemical property is observed when a substance interacts with another substance. Burning or flammability RustingTarnishing Whether an object will explode Chemical Properties

30. Elements and their Properties

31. Two major groups of elements Found on the periodic table Metals are located to the left of the zigzag line Nonmetals are located to the right of the zigzag line

32. Physical Properties of Metals Have Luster -shiny Are Conductors -heat and electricity move through them easily Malleable – Can be hammered into a different shape Ductile – Can be drawn into a wire High Density – Heavy for their size Metals are solid, except for mercury

33. Alkali Metals Group 1 on the periodic table Shiny, malleable and ductile Good conductors of heat and electricity Highly reactive metals

34. Transition Elements Groups 3 – 12 Less active than groups 1 and 2

35. Physical Properties of NonMetals Dull – not shiny Nonconductors – heat and electricity do not move through easily Brittle – break easily Most nonmetals are gases at room temperature

36. Metalloids Both metal and non metal May conduct electricity better than many nonmetals but not as well as some metals

37. Solutions Two (or more) substances mixed so thoroughly that neither can be observed in its original form. Homogenous mixture, in which the particles of the mixing substances are evenly distributed throughout 1) Salt water 2) Syrup (sugar in water) 3) Vinegar (acetic acid in water) 4) Shampoo (various soaps and surfactants dissolved in water) 5) Oxygen 6) Brass

38. Solute vs Solvent The substance being dissolved is the solute The substance that dissolves the solute is the solvent

39. 3 Types of Solutions GaseousLiquidSolid

40. How Do you Increase Rate of Dissolving? For most solids Increase temperature StirShake Break solute into smaller pieces

41. Solubility Different solutes dissolve at different temperatures Solubility: the maximum number of grams of the substance that will dissolve in 100g of solvent at a certain temperature Saturated solution: a solution that has dissolved all the solute it normally can hold at a given temperature Oversaturated solution: any solution that can dissolve more solute at a given temperature Supersaturated: Contains more solute than a saturated one has at that temperature. Unstable solution

42. Barrons p 240