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1St Halfchemnotes Science 10 Chemistry Notes Matter and Classification Purpose of classification: to gain a better understanding and appreciate similarities or differences Matter: Has mass and occupies space. We can divide matter into two categories as follows: Matte Pure Mixtur Heterogeneo Homogeneo Elemen Alloy Solutio Metal Nonmeta Compou Ioni Molecul PURE SUBSTANCES Substances that are the same or consistent throughout. Can be a single element or a combination of elements. Elements: Substance composed of only one kind of atom. 109 on the periodic table. Each has a unique international symbol. Can be combined to make other pure substances. Compound: Combination of two or more elements in specific proportions. Once combined the compound acts as one, with consistent chemical and physical properties. Chemical vs. Physical Properties Chemical - describes the reactivity of a substance. Physical -no new substance formed. Has similar properties in each form. Usually a change in phase. ie. Liquid, solid or gas. Chemical Reactions The process that occurus whena subtance or substances reacts to creat a different substance. - involve the production of new substances - involve the flow of energy (exothermic and endothermic) - involves formation of a gas - involves the formation of a solid in a liquid Periodic Table Elements on the periodic table are classified and arranged according to four basic patterns: 1. Atomic number: the number of protons (positively charged particle) in the nucleus of an element. The number of electrons in an atom 2. Metals vs. non-metals: separated by the staircase line. 3. Groups (or families): vertical columns that have similar properties. 4. Periods: horizontal rows which indicate the number of electron shells an atom has. Example : Calcium: atomic number __________ metal/non-metal___________ group ______________ period________________ The periodic table can also list the physical state (phase) of the element at room temperature. Regular Print - solid Clear Print - gas Bold- liquid- There are only two (Hg, Br) Chemical Families Group 1 Alkali metals Elements are highly reactive. Contain most reactive metal: Francium. Silver colored Very ductile React with air or water Group 2 Alkaline Earth Metals Similar to alkalies but not as reactive in air. Oxidize with air to form a protective coating Group 17: Halogens - “Salt Formers” Reacts well with metals to form compounds similar to salts. Most diverse Group. Contains all phases. Contains most reactive non-metal: Fluorine Group 18: Noble Gases Seldom reacts to form compounds. formerly called the “Inert Gases” Group B elements: Transition Metals typical metals such as copper, iron, zinc and silver wide variety of characteristics Metal are seperated from the Non-Metals by the staircase Metal vs Non-Metal Properties Metals Non-Metals -solid (except Hg) -s, l, g -silver(except: copper, gold) -all colors -ductile & malleable -no -conduct heat/electricity -no -reacts with acid to form -some hydrogen gas Metalloids -Nonmetals along the staircase line that have some of the properties of metals, mainly they can conduct electricity. (semiconductors) Last Two Groups - found at the bottom of the periodic table Rare Earths / Lanthanide Series: Name says it all, atomic #’s 58 - 71 Trans Uranium /Actinide Series: Made in nuclear reactors, #’s 90-103 Atomic Structure Atom: The basic unit of matter. Smallest unit of matter that retains the properties of the element. Atom has a specific structure of subatomic particles consisting of: 1. Proton: symbol “p+” -Positively charged particle located in the center of an atom (nucleus). Makes up a large portion of the mass of an atom. 2. Neutron: symbol “n°” -Neutral charged particle located in the center of the atom(nucleus). Also makes up a large portion of the mass of the atom ***Atomic mass of any element is determined by the number of protons and neutrons. 3. Electron: symbol “e-” -Negatively charged particle surrounding an atom. -Has very little mass. Moves about the nucleus in an electron cloud. Cloud consists of mostly space. If the nucleus was the size of a ping pong ball the first electron would be about 0.5 km away! Finding Numbers of Subatomic Particles Protons = Atomic Number *Proton number can never, never, never change. Electrons = Atomic Number (neutral atom only!) *Electron number can change. Neutrons = Mass number - Atomic number. Isotopes: Atoms that have a different number of neutrons from another atom of the same element. U 235 is a light isotope having 3 fewer neutrons than the most common form of uranium U 239 is a heavy isotope having 1 more neutron than the most common form of uranium The Development of an Atomic Model As theories developed old ideas were not discarded, they were modified and expanded upon. Dalton “Billiard Ball” Model Atom is in the shape of a billiard ball and acts as a single, indestructible and indivisible particle. The larger the atomic number the larger the atom or “billiard ball” Observations that supported this theory: Law of Conservation of mass: The masses of the reactants always equals the masses of the products. Example: 2 g of hydrogen and 16 g of oxygen would react to produce 18 g of water. J.J. Thomson “Raisin Bun” Model Atoms have negatively charged particles embedded in them like raisins in a bun. Observations that supported theory: -electricity passed through a gas in a vacuum tube produced a stream of negatively charged particles. Rutherford “Nuclear” Model An atom’s mass is concentrated in a very small,dense and positively charged nucleus. Electrons orbit the nucleus at a distance. Observations that supported theory: Gold foil experiment- large positively charged particles should go right through the gold foil. Most did but some came right back towards the particle emitter. Bohr “Solar system” Model Electrons are located in specific orbits, each having a specific energy level, around the nucleus. It is the electrons in the outermost orbit that react with neighboring atoms to form compounds. Observations that supported theory: electricity passed through a gaseous element emits only certain wavelengths of light. Quantum Mechanical Model “Electron Cloud Model” Electrons are in a cloud moving very quickly around a nucleus forming an electron cloud. Atoms and Ions Ions: charged particles (atoms) that have lost or gained electrons. They lose or gain electrons in order to have an electron structure similar to that of a Noble gas. Reason: Noble gases are stable!! Comparing atoms to ions. Atoms Ions -neutral charge -positive or negative charge -# of electrons equal -# of electrons different from to atomic number the atomic number (# of protons) -protons equal atomic number -protons equal atomic number Bohr Diagrams # of protons goes in the nucleus # of electrons can be distributed as follows: maximum of 2 e- in the first level maximum of 8 e- in the 2nd level maximum of 8 e- in the third level Draw a Bohr diagram for sodium and for fluorine. METALS: -Tend to lose electrons. -They become positively charged and are called cations. -The size of the positive charge is determined by the number of electrons lost. -The number of electrons lost is determined by the proximity to the nearest Noble gas. -Named by using the full metals name and adding ion at the end. Ex: Magnesium is a group two element. An atom of magnesium has ____ electrons. The nearest Noble gas is ________ and it has ______ electrons. An ion of magnesium must also have _______ electrons because this is a more stable configuration. This results in magnesium having a net charge of 2+. It is named ___________________ NON-METALS: -Tend to gain electrons. -They become negatively charged and are called anions. -The size of the negative charge is determined by the number of electrons gained. -The number of electrons gained is determined by the proximity of Noble gas. -Named by dropping the ending and adding an ‘ide’ ending Ex: Chlorine is a group 7 element. An atom of chlorine has _______ electrons. The nearest Noble gas is ________ and it has ______ electrons. An ion of chlorine must also have _______ electrons because it is more stable. This results in chlorine having a net charge of 1-. The name is ___ IONIC COMPOUNDS Metals lose electrons to form positively charged ions called cations. Nonmetals gain electrons to form negatively charged ions called anions. When metals react with nonmetals an exchange of electrons occurs resulting in two oppositely charged ions. It is these charges that cause the bond to form because opposite charges attract. The result is a crystal lattice. Properties of ionic compounds: - solid at room temperature - dissolve in water (soluble) to form solution - solutions conduct electricity (electrolytes) - solutions can be any color - have higher melting & boiling points Charges must balance because one element gives up electrons and the other one accepts these same electrons. The formula is the ratio of one ion to another. Example 1: Sodium atoms tend to lose an electron to form the cation, Na1+. Chlorine atoms tend to gain electrons to form an anion, Cl1-. When these two elements are brought together under the proper conditions a chemical reaction takes place in which the sodium atom gives its electron to the chlorine atom. These two ions attract each other and form a new compound, NaCl (s). Name the compound by using the full name of the metal followed by the name of the nonmetal with the ‘ide’ ending. The above compound,NaCl (s), is named sodium chloride. Sometimes more than one ion is required to react with another ion. Example 2: Calcium reacts with fluorine. First, determine the charge on the ions. Look up each element on the Table. Ca2+ and F1-. Calcium tends to lose two electrons but fluorine can only accept one. It takes two fluoride ions to react with the calcium ion so the resulting compound is CaF2 (s).
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