Chemistry CHEMISTRY NOTES Atom- Element- Compound- Molecule- The building blocks of matter Made of protons, neutrons and electrons. Pure substances that cannot be separated. Ex: Gold 2 or more elements bonded together Ex: CO2 Smallest part of a compound that still has the same properties Example: Hydrogen (H) and Oxygen(O) are Elements. When 2 atoms of hydrogen and atom of oxygen combine they form molecule of the compound water (H2O).
SUBATOMIC PARTICLES Atoms are made up of 3 subatomic particles. In the nucleus (core or center of the atom) there are 2 particles. Protons + charge.. Subatomic particles with a Neutral Neutrons No charge, or. 2. Subatomic particles with a The 3rd subatomic particle orbits (flies around) the nucleus. Electron Negative 3. Subatomic particles with a charge. THE PERIODIC TABLE Mendeleev Developed by in the 800s. Elements ) Lists all of the. 2) From left to right the elements are listed in increasing atomic number. periods 3) The rows (Horizontal) are called. (Get it? Like PERIODic table!) All these elements have the same amount of electron shells. (Which we will discuss later.) groups or families Elements in the same 4) Columns (Vertical) are called. group have similar properties. Symbols- either capital letter or capital letter combined with a lowercase. H ex: Hydrogen- He Helium
USING THE PERIODIC TABLE The periodic table contains 2 main numbers. ) The Atomic Number- the number of Protons in an atom. This determines what element it is. No two elements have the same atomic number. Because atoms are neutral it is also the number of. Electrons Protons Neutrons 2) Atomic Mass- the total number of & in an atom. Basically the total mass of an atom Mass of an atom Because atoms are so small, scientists had to create a new unit to measure their mass. The Atomic Mass Unit or AMU. In this system the mass of a 2.0 6 CCarbon Proton = AMU Neutron = AMU Electron = 0 AMU 2-4 To find the number of protons, neutrons, electrons: ) The # of protons = the atomic number 2) The # of electrons = the atomic number 3) The # of neutrons = Round the atomic mass, then - atomic # 5.9994 8.9994 96.967 4.002 O F Au He 8 Oxygen 9 Flourine 79 Gold 2 Helium 2-6 2-7 *32-8- 2 # P= 8 # P= 9 # P= 79 # P= 2 # E= 8 # E= 9 # E= 79 # E= 2 # N= 8 # N= 0 # N= 8 # N= 2
Why aren t atomic masses whole numbers? Answer: Atoms come in different forms. These different forms are called isotopes. The atomic mass is an average of these atoms. Isotopes: Atoms of the same element that have a different number of neutrons. ISOTOPES OF CARBON
More Practice 39. K Potassium 9 2-8-8-27.0 Al Aluminum 3 2-8-3 Symbol: K Name: Potassium Atomic number: 9 Atomic mass: 39 # protons: 9 # neutrons: 20 # electrons: 9 79.9 Symbol: Br Br Bromine Name: Bromine Atomic number: 35 Atomic mass: 80 # protons: 35 35 2-8-8-7 # neutrons: # electrons: 45 35 Symbol: Al Name: Aluminum Atomic number: 3 Atomic mass: 27 # protons: 3 # neutrons: 4 # electrons: 3 Drawing Atoms. Calculate the # of p, e & n 2. Draw a circle for the nucleus 3. Inside the nucleus write the number of protons and neutrons. 4. Draw a circle around the nucleus for each electron shell. 5. Fill in the amount of electrons for each orbit. 27.0 +3 Al Aluminum 3 2-8-3 8.9-9 2-7 F Flourine 24.2 +2 Mg Magnesium 2 2-8-2 P = 3 N = 4 P = 9 N = 0 2 7 P = 2 N = 2 2 8 2
Drawing Atoms (Electron Dot Diagrams). Write the element s symbol. 2. Put dots on each side of the symbol to represent the outer shell. 3. Begin on the top - right - bottom - left then back to the top. 27.0 +3 Al Aluminum 3 2-8-3 8.9-9 2-7 F Flourine 24.2 +2 Mg Magnesium 2 2-8-2 Al F Mg Compound Notes 2 or more elements joined together # of molecules 4H2O Compound- Coefficient- Subscript- How many atoms of an element there are Subscripts and coefficients making equations easier & neater. Rewrite 4H2O without a coefficient: H2O H2O H2O H2O Rewrite 4H2O without a subscript: 4HHO
Breaking Down a Compound Ex: Al2O3. List the elements. 2. How many molecules are listed? 3. Determine the total # of atoms of each element. Al O # Molecules # Atoms = 2 2 3 3 Parentheses: (NO3)3 -st subscript is applied to oxygen only -2nd Subscript is applied to The entire molecule Ex: 3H2(CO3)3. List the elements. 2. How many molecules are listed? 3. Determine the total # of atoms for each element H #Molecules x # Atoms = 3 2 6 C 3 3 9 O 3 9 27
I know how much atoms weigh but, what about Compounds?. Fill in the symbols column (b) 2. Fill in the amount of molecules (c) 3. Fill in the # of atoms (d) 4. Look up the atomic mass using your periodic table and place it in column (e) 5. Multiply the # of atoms by their atomic mass (f) 6. Add the atomic masses together to get the total molecular mass (g) (a) Compound (b) Symbol (c) # Molecules (d) # atoms (e) Atomic Mass (f) (g) Total Mass Na(NO3) Na N O 3 23 4 6 23 4 48 85 AMU HCl H Cl 35 35 36 AMU (a) Compound (b) Symbol (c) # Molecules (d) # atoms (e) Atomic Mass (f) (g) Total Mass CO2 C O 2 2 6 2 32 44 AMU 4C2H22O C H O 4 48 88 44 2 6 576 88 704 368 AMU 6H2SO4 H S O 6 2 6 24 32 6 2 92 384 588 AMU 3Ni(ClO3)3 Ni Cl O 3 3 9 27 59 35 6 77 35 432 924 AMU
HOW COMPOUNDS ARE MADE All atoms want thing... to be. Stable STABLE is having 8 electrons in the outermost shell. Atoms can accomplish this by gaining or losing electrons. OCTET RULE: Atoms will form compounds to reach eight electrons in their outer energy level. Atoms with less than 4 electrons in their outer level tend to lose electrons to form compounds. Atoms with more than 4 electrons in their outer level tend to gain electrons to form compounds. Valence Electrons Electrons in the outermost shell are known as. All Members of a group have the same Valence number! Outermost shell Valence Electrons are the electrons found in the. Electron Shells 0.8 +3 B 5 Boron 2-3 Oxidation Number 79. - Br 35 Bromine 2-8-8-7 Electron Shells Valence Electrons
Outermost energy level Na Sodium 2-8- Sodium has valence electron. Sodium s oxidation number is. + Sodium can have 8 electrons in its outer shell if it loses (lends) an electron. Cl Chlorine 2-8-7 7 Chlorine has valence electrons. Chlorine s oxidation number is - The - means sodium wants to gain (borrow) one electron than have 8 electrons in its outer shell. C Carbon 2-4 4 Carbon has valence electrons. +4 or -4 Carbon s oxidation number is. Ga Gallium 2-8-8-3 3 Gallium has valence electrons. Gallium s oxidation number is. +3 It has 3 extra electrons to lose to become stable.
Using your Periodic Table fill in the chart. Element Valence Electrons Oxidation Number Potassium Calcium Lead Krypton Phosphorus + 2 +2 4 +4 / -4 8 0 5-3 Element Valence Electrons Oxidation Number Zinc 2 +2 Lithium + Manganese 2 +2 Nitrogen 5-3 Silicon 4 +4 / -4 Sulfur 6-2 Barium 2 +2 Nickel 2 +2 Copper +
Forming Compounds Water s formula is always H2O because H has electron to lose, but Oxygen needs 2 electrons. So 2 H s each share electron with Oxygen! + + -2 H + H + O = total net charge of 0 We use the criss-cross method as a short cup to determine the chemical formula for a compound. Here are the steps:. Write down the oxidation numbers. Metals are always written on the left and nonmetals on the right. 2. Criss-cross the oxidation numbers to make them the new subscript for the element. Ex: + -2 H O 2 3. Write the formula = H2O 4. Reduce or rewrite the formula. ( is not written) H2O
Determining compound formulas. Write the symbol of the metal on the left and the nonmetal on the right. 2. Find the oxidation number on the periodic table. 3. Criss-cross the oxidation numbers, drop the sign. 4. Do not write ones. Examples: Sodium and Phosphorus Na + -33 P Calcium and Sulfur Ca +2-22 S Na3P Ca2S2 CaS Practice forming compounds. Beryllium + Fluorine Be +2 - BeF2 F 2. Magnesium + Oxygen 3. Barium + Chlorine Mg Ba +2 Mg2O2 MgO O -22 +2 - BaCl2 Cl
Metals vs. Nonmetals Metals Less than 4 electrons in outermost shell Wants to lose extra electrons Nonmetals More than 4 electrons in outermost shell Bismuth (Metal) Wants to gain electrons to fill outermost shell Has a + oxidation # Has a - oxidation # Are malleable and ductile Are brittle Sulfur (Nonmetal) Metals usually link up with nonmetals to form compounds. Metallioids- properties of both metals and nonmetals found along the stair-step Ex: B, Si, As, Ge, Sb, Te, At Metals vs Nonmetals Metalloids Metals Nonmetals
Radicals Radical- A group of atoms that act like a single atom. Radicals always act like one atom. They have their own oxidation number. You can look these up on your list. Radicals can form compounds, use the same steps to determine the formula. Just keep the radical in the parenthesis (). Examples: Ni (PO4) (NH4) (CO3) Ni +2 2-33 (PO4) + -22 (NH4) (CO3) Ni3(PO4)2 (NH4)2 (CO3)