Chapters 1 & 2 Atoms and Elements and Chemical Reactions (Period 5) CHEMISTRY REVIEW

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1 Chapters 1 & 2 Atoms and Elements and Chemical Reactions (Period 5) CHEMISTRY REVIEW

2 T = CHAPTER 1 ATOMS AND ELEMENTS Elements and Atoms Matter - anything that takes up and has mass Elements A substance that cannot be broken down into any other substance Compound a substance made of two or more elements that is combined chemically in a specific ratio. Mixture when two or more substances are combined-non chemically (dirt, air, mulch, fish in water, mud) Atom the smallest particle of an element

3 T = CHAPTER 1 ATOMS AND ELEMENTS Atomic Theories Daltons - composed that atoms can not divided, they are all alike, every compound is made of atoms in specific ratios, atoms can not be created or destroyed. Thomson chocolate chip cookie model (electrons are everywhere) Rutherford - Gold foil experiment (the existence of a nucleus) Bohr onion orbitals (looks like the planets orbiting the sun which would be the nucleus and planets are the electrons in the orbits Cloud electrons can be anywhere Modern (Chadwick) - neutrons

4 T = CHAPTER 1 ATOMS AND ELEMENTS Elements and Periodic Table Period horizontal Group (family) column- vertical Metals most of the chart until Group 13 Non Metals Groups Semi Metals Staircase Atomic Number number in the box= # protons if neutral = # of electrons Symbols the shortened version of an element ex. Oxygen = O, Lithium = Li, Sodium = Na, Sulfur = S Valence Electron Electrons on on the outer orbital. They have the highest energy level. Gr. 1 and 2 like to give up electrons because losing 1 or 2 electrons is the easiest way to be KING(noble gases). Halogens like to take electrons to gain noble status.

5 T = CHAPTER 1 ATOMS AND ELEMENTS Elements and Periodic Table Metals - luster, malleable, ductile, conducts heat, conductive, sea of electrons Semi Metals can exist as both a metal or a non metal depending on temperature, what it is paired with! Non Metals - all non metals have at least four valence electrons and Halogens become stable when they gain or share electrons Electron Dot Structure shows the number of valence electron as dots around the symbol Atomic Orbital Structure - p/n in middle, layer like an onion or planets, circles. First orbit has 2, all others filled up to 8. The outermost circle holds the valence electrons

6 T = CHAPTER 1 ATOMS AND ELEMENTS Group Names Alkali Metals Group 1 Alkaline and Earth Group 2 Halogens Group 17 Nobel Gases Group 18 Covalent Bonding Share electrons Usually Form between non metals Become more stable when they share Non Polar Electrons shared equally Polar Electrons shared unequally Single Bonds 2 electrons Double Bonds 4 electrons Triple Bonds 6 electrons Do not conduct electricity

7 T = CHAPTER 1 ATOMS AND ELEMENTS Ionic Bonding Transfer of electrons Always polar Bond is due to the attraction of the opposite charges Form crystals High melting points Conduct electricity Metallic Bonding Attraction between a positive metal ion and the electrons surrounding it Consists of a positively charged metal ion embedded in a sea of electrons Alloy material made of two or more elements that have the characteristics of a metal Every metal ion is held by a metallic bond Conduct Heat and Electricity Lust and Malleability and ductility

8 CHAPTER 2 OBSERVING CHEMICAL REACTIONS T= Observing Chemical Change Properties and Changes of Matter Physical Properties Observable change without changing the substance Ex squishing, vaporization, Change of state, Chemical Properties Observable change which DOES change the substance into another substance Ex. Fire(burning), oxidized, rusted, tarnish Physical Change A change in its state but the substance is not changed Chemical Change Changing the substance into another substance

9 T= OBSERVING CHEMICAL CHANGE Evidence for Chemical Reactions Sensing a change in smell See a precipitate Solid formed from two liquids Change of heat/temperature Exothermic release of heat (feels hot) Endothermic absorbing heat (feels cold) Change of color

10 T= DESCRIBING CHEMICAL CHANGE Chemical Equation Reactant + reactant YIELDS Product + Product Short easy way to show a chemical reaction using symbols Yield = arrow Product is the end solution/material/substrate Reactants are the substances in the beginning Coefficient is the number in front which represents the number of molecules of that particular substance Conservation of Mass The principal stating that matter is not created nor destroyed during a chemical reaction Closed System Where substances can not come in or be let out! Balloon, air bag(partial), class jar with lid, zip lock bag, sealed box, Open System System in which matter can enter and or escape Beaker (open), campfire, cooking pot

11 T= DESCRIBING CHEMICAL CHANGE Balancing Chemical Equations Both sides have the same number of each type of atom. Write the equation Count the atoms (on each side) Use coefficients to balance the atoms Look Back and Check

12 T= CLASSIFYING CHEMICAL REACTIONS Replacement - Switch Partners Synthesis Simple to Complex Decomposition - Complex to Simple

13 T= CONTROLLING CHEMICAL REACTIONS Temperature Surface Area Simple to Complex Concentration - Complex to Simple Inhibitor - Slows down a reaction Catalyst Speeds up a reaction

14 T= CONTROLLING CHEMICAL REACTIONS Temperature - adds or removes energy increased temp increases the reaction rate. Surface Area greater surface area increases the reaction Concentration higher concentration usually increases the reaction rate Inhibitor - Slows down a reaction Catalyst Speeds up a reaction

15 T= FIRE AND FIRE SAFETY Temperature - adds or removes energy increased temp increases the reaction rate. Surface Area greater surface area increases the reaction Concentration higher concentration usually increases the reaction rate Inhibitor - Slows down a reaction Catalyst Speeds up a reaction

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