Lots of examplesKClPotassium chlorideMg3N2Magnesium nitrideNa2SO4Sodium sulfate(NH4)2CO3Ammonium carbonateCuOCopper(II)oxideCu2OCopper(I)oxideFePO4Iron(III)phosphateįormula Writing Ionic CompoundsIdentify the compound as ionicFind the formula and charge of the cation and the anion.Use subscripts to indicate the number of each ion needed to have an overall neutral charge. Then write the name of the anionPolyatomic anions are simply namedRemember the name of a monatomic anion ends in ide.oxygen forms the anion oxide (O2-)nitrogen forms the anion nitride (N3-) Naming Ionic CompoundsSimply write the name of the cation firstGroup 1,2 elements, Al3+, Zn2+, Ag1+, Ga3+, In3+ are simply named Polyatomic cations are also simply namedOther metals can have more than one charge, so the name must indicate the charge with a roman numeral.Cu1+ is copper(I)Cu2+ is copper(II) Ionic CompoundsAre formed because of the strong electrostatic attraction between cations and anions.Binary ionic compounds are always between a metal and a non-metal.Other ionic compounds must contain a polyatomic ionExamples: Table salt (NaCl), baking soda (NaHCO3), Epsom salts (MgSO4) Charge related to position on Periodic Table for monoatomic ionsCation: Positive ion (Typically metal)Anion: Negative ion (Typically non-metal)īackground: FormulasEmpirical formula: shows the lowest whole number ratio of the atoms in the compound.Molecular formula: shows the exact number of each kind of atom in the compound.Structural formula: shows how the atoms in the molecule are bonded togetherīackground: Formula of Molecular Compoundsīackground Practice: BenzeneStructural Formula?Molecular Formula?Empirical Formula Typically a covalent bond is between two non-metals (This is a general rule of thumb.)Įxamples: Water (H2O), Bromine (Br2), ammonia (NH3), Vinegar (HC2H3O)īackground: IonsDefinition: An atom or group of atoms that have an overall positive or negative chargeMonatomic ions: atoms that have lost or gained electrons. Some of the groups in the periodic table are given special names.These names indicate the similarities between group members:Group 1: Alkali metals.Group 2: Alkaline earth metals.Group 16: Chalcogens.Group 17: Halogens.Group 18: Noble gases.Background: Periodic Tableīackground: MoleculesDefinition: a group of two or more atoms held together by a covalent chemical bond. (Assume that the masses are 107.00 and 109.00 respectively.) Calculate the percentage of each isotope in naturally occurring silver. Silver consists of two isotopes 107Ag and 109Ag.
Isotope Calculations Example 1Using the isotope information for Silicon. Isotope Calculation ReviewThe atomic masses listed on the periodic table are average atomic massesThey are determined by calculating the weighted mean.Īverage atomic mass = (isotope mass)( relative abundance) Isotopes, Atomic Numbers, and Mass NumbersĪtomic number (Z) = number of protons in the nucleus.Mass number (A) = total number of nucleons in the nucleus (i.e., protons and neutrons).By convention, for element X, we write ZAX.Isotopes have the same Z but different A.
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