Your Guide for Success Chemistry Unit Name:
Chemistry Outline I. Atoms A. Structure of an Atom 4 1. Subatomic Particles 2. Different Form b. Isotope II. Periodic Table 1. Arranging 6 a. Mendeleev b. Mosely 2. Grouping the Elements 8 III. Chemical Bonding A. Ionic Bonding 10 1. Forming Ionic Bonds 2. Forming Positive Ions 3. Forming Negative Ions 4. Properties B. Covalent and Metallic Bonds 12 1. Molecules 2. Movement of Electrons in Metallic Bonds 3. Properties of Metallic Bonds 1V. Chemical Reactions A. Forming New Substances 14 B. Chemical Formulas and Equations 16 1. Chemical Formulas 2. Writing Formulas for Covalent and Ionic Compounds 3. Chemical Equations 4. Law of Conservation of Mass 5. Balancing Equations 2
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The Atom vs. The Isotope Chapter _4_ Section _2_ Pages _88-94_ Smallest unit of an that maintains the properties of that element. Contains subatomic particles: Protons,, and Electrons Electron Cloud: the nucle- Nucleus: Tiny, core of an atom us Most of an atom s Contains and neutrons Most of an atom s. Contains Very small and. charged Protons: charged 1 = 1 amu Atomic # = the number of Symbol: + or Neutrons 1 = 1 amu Symbol: 0 or MUCH VERY # of Electrons = # of Symbol: - or Together: Protons + = atomic mass An that has the same number of (atomic number) but a number of, therefore it has a different 4
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Arranging the Elements Chapter _5_ Section _1_ Pages _106-112_ History 101-The Periodic Table Dmitri Mendeleev Chemist Discovered a in the elements properties. His final arrangement increasing atomic. He left gaps in the his table for yet elements. He could the properties of the undiscovered elements. Our Current Periodic Table Henry Mosely Scientist Rearranged original table Our current periodic table is by atomic. This allowed all elements to fit the. Classification of Elements on the Periodic Table Metals of zig-zag line Metalloids zig-zag line Nonmetals of zig-zag line valence electrons About a complete set of valance electrons or almost complete set of valence electrons An element s classification is determined by its number of electrons. The line helps you recognize where to locate each classification on the Periodic Table. Decoding The Elements of the Periodic Table Periods Direction = Period # = There are periods. Groups/Families Direction = Each group has properties. If you know the group number you can determine the number of electrons. There are groups. 6
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Grouping the Elements Chapter _5_ Section _2_ Pages _114-120_ Group 1 (G1) Alkali Metals: reactive metals Group 2 (G2) Alkaline-Earth Metals: reactive than G1 1 electron 2 electrons Often store in Found in nature in Physical Properties Soft,, shiny, and low Physical Properties Silver, density than G1 Used in manufacturing Found in and cement Groups 3-12 (G3-12) Transition Metals: 1 or 2 electrons (Do not let them go as easily as G1 or G2) Less than G1 and G2 Good density, melting point than G1 and G2 Lanthanide Series: Appears at the bottom of the table to keep it from being too wide. Actinide Series: /Unstable After element number made in laboratories. Group 13 (G13) Boron Group: metalloid and metals 3 electrons at RT Most common = Group 14 (G14) Carbon Group: nonmetal, metalloids, and metals 4 electrons Varying at RT Used in chips 8
Grouping the Elements..continued Chapter _5_ Section _2_ Pages _114-120_ Group 15 (G15) Nitrogen Group: nonmetals, metalloids, and metals 5 electrons % of the gas we breathe. reactive Group 16 (G16) Oxygen Group: nonmetals, metalloids, and metals 6 electrons % of the gas we breathe. Groups 17 G(17) Halogens: All 7 electrons Very Need to gain only valence electron Forms compounds with very easily. Chemical properties Physical properties different Group 18 (G18) Noble Gases: All Hydrogen: 8 electrons Exception is He valence electrons. STABLE! 1 electron Set a part because the do not any other group. Is placed above because the of valence electrons is the same. Most element 9
Ionic Bonding Chapter _1_ Section _2_ Pages _8-11_ Ionic Compounds Forms when electrons are transferred (gained or lost) from one atom to another to each others outer energy level. Forms between (+ ions) and nonmetals ( ions) When formed, the # of lost equals the # of electrons. Therefore, ionic compounds are. The charges each other out. Properties include; bond, melting and boiling points. Writing Ionic Formulas Always write the ion or first. Write the ion or the second. Polyatomic ion an ion that is made up of more than one atom (2 capital letters Ex (NH 4 ) + When written name remains the same. Use parentheses numerals show number. An oxidation number is the number of electrons an atom gains or loses to become. Make sure compounds are. Forming + Ions - Cation Forming - Ions Anion Occurs when an atom valence electrons. An atom now has protons than negative electrons. (Unbalanced + and -) form + ions because they have valance electrons (1, 2, or 3) Only takes a small amount of to lose their few electrons. and are examples of atoms that form + ions. Occurs when an atom valence electrons. An atom now has move electrons than positive protons. (Unbalanced + and -) form - ions because they have an almost full outer level. Ending of the elements name changes to (Ex. Fluorine >Fluoride) and are examples that form - ions. 10
Section A: Complete the chart using a periodic table to help you. Section B: Answer these questions: 1. An atom that gains one or more electrons will have a charge. 2. An atom that loses one or more electrons will have a charge. 3. At atom that gains or loses one or more electrons is called an. 4. A positive ion is called a and a negative ion is called a. 5. Atoms will transfer one or more to another to form the bond. 6. Each atom is left with at outer shell. 7. An ionic bond forms between a ion with a positive charge and a ion with a negative charge. Section C: Draw the ionic compounds below. Show the transfer, give the name of the compound and give the formula. Example #1: Sodium + Chlorine Example #2: Magnesium + Iodine Example #3: Sodium + Oxygen Example #4: Aluminum + Chlorine 11
Covalent and Metallic Bonding Chapter _1_ Section _3_ Pages _12-17_ Covalent Molecules Forms when atoms valence electrons to complete an atom s outermost energy level. Forms between 2 or more. May have bonds between the atoms. Consist of individual particles called. Simplest type = Example Hydrogen H 2 and Oxygen O 2 Properties: bond, melting and boiling points. Metallic Compounds This type of bond is formed by the between positively charged metal ions and the in the metal. The metals outermost energy levels. This overlapping allows the electrons to move throughout the metal. The cancel the charge of the ions. Writing Covalent Formulas Usually the name tells you the. However, many molecules have names Example dihydrogen monoxide = water Pay attention to used. Mono Hexa Di Hepta - Tri Octa - Tetra Nona- Penta Deca Properties of Metals Metallic bonding is what gives their particular properties. When metals are electric current, the electrons are moving through the metal. Because of the electrons, metals may be. Malleability and describe how a metal may be reshaped. 12
Section A: Answer these questions: 1. Atoms one or more electrons with each other to form the bond. 2. Each atom is left with a outer shell. 3. A covalent bond form between two. Section B: Draw the molecular compounds below. Show how they share, give the name of the molecule and give the formula. Example #1: Hydrogen + Hydrogen Example #2: Hydrogen + Oxygen Example #3: Chlorine + Chlorine Example #4: Oxygen + Oxygen Example #6: Carbon + 4 Hydro- Example #5: Carbon + 2 Oxygen gen Write the formulas for the following covalent compounds: 1) antimony tribromide 2) hexaboron silicide 3) chlorine dioxide 4) hydrogen iodide 5) iodine pentafluoride 6) dinitrogen trioxide 7) ammonia 8) phosphorus triiodide Write the names for the following covalent compounds: 9) P 4 S 5-10) O 2 11) SeF 6 12) Si 2 Br- 6 13) SCl 4 14) CH 4 15) B 2 Si 16) NF 3 13
Forming New Substances Chapter _2_ Section _1_ Pages _28-31_ Chemical Reactions A process in which one or more substances to make one or more substances. The and physical properties from the original substances. Some Signs of Chemical Reactions Reactions often have more than one of these signs. And the more of these signs you see, the more likely that a chemical reaction is taking place. However there is NO guarantee. The MOST important sign is of a substance! How do new substances form in a chemical reaction? Chemical bonds in the original substances must. The rearrange. New form to make substances. 14
On your desk place the Physical Change card to your left and the Chemical Change card to your right. Using what you know about physical and chemical changes, place each card into the correct category. Record you data in the chart below. Physical Change Chemical Change Were there any cards you had trouble classifying? Give an example of a physical change that was not listed above. Give an example of a chemical change that was not listed above. 15
Chemical Equations Chapter _2_ Section _2_ Pages _32-36_ Use symbols and to describe a chemical reaction. Starting materials = Ending materials = Accuracy is key when writing chemical equations! Equations MUST BE Balanced! Atoms are never or gained in a chemical reaction just. The of reactants must equal the number of. Based on the work of Antoine Lavoisier Law of of. Steps to balance a chemical equation. 1. Write symbols and correctly. 2. Make 2 lists of - write it the on both sides of the arrow. 3. Count 4. Use to balance 5. Recount/ if necessary. Never Ever Balance by Changing a Subscript! 16
Balancing Equations Practice Part A: Identify the following parts of each chemical formula by circling the subscripts and drawing a square around the coefficients. H 2 2HCl 4O 2 CH 4 3CO 3 2NaOH Part B: List the symbols for the atoms in each formula and give the number of each. C 2 H 6 2MgO 4P 4 O 10 NH 3 3Al(OH) 3 2H2O Part C: Balance each of the following equations following the procedure described in class. Be sure to show your work. P + O 2 P 4 O 10 Mg + O 2 MgO P = P = Mg = Mg = O = O = O = O = HgO Hg + O 2 Al 2 O 3 Al + O 2 Hg = Hg = Al = Al = O = O = O = O = BaCl 2 + H 2 SO 4 BaSO 4 + HCl Ba = Ba = Cl = Cl = H = H = S = S = O = O = 17