Chemical Reactivity – How much an element reacts depends on the electron configuration of its atoms. › Ex: O and Ne Noble gases are least reactive. Alkali metals and halogens are most reactive. WHY?
Group number tells you how many electrons are in an element’s valence shell. Atoms gain and lose electrons to become stable.
An atom and its ion have different chemical properties. › Stable ion should not be confused with noble gas Has a charge now and forms a compound.
Atoms of metals & nonmetal elements form Ions differently. › Almost all metals form cations Ex: Mg – 1s2 2s2 2p6 3s2 Takes less energy to lose 2 electrons, than gain 6. Nonmetals form anions › Ex: O – 1s2 2s2 2p4 › Gaining 2 electrons requires less energy than losing 6.
Form between ions of opposite charges (+ & -). › Compound becomes electrically neutral. › Ex: NaCl
Ionization energy – energy needed to remove the outermost electron from an atom. Endothermic – Needs energy to be put in the reaction in order for the reaction to occur. Exothermic – Reaction releases energy (often heat).
Strong Have high melting/boiling points Rarely gas at room temp. When dissolved conduct electric current. Salts are hard and brittle.
Simple Ions: › Cation borrows name of element: K is potassium ion. › When element forms 2+ ions, roman numerals are used: Ex: Cu+ : copper (I) ion Cu 2+ : copper (II) ion › Anion also uses element name but, add ide to end. Ex: chloride, oxide
Cation name followed by anion › Ex: NaCl sodium chloride › Ex: Mg3N2 magnesium nitride › Ex: K2 potassium oxide
Must have no overall charge (neutral). › Ex: Mg 2+ and N3-
Presence of Oxygen – ite and -ate. The one with less O is ite, while the one with more O is ate. › Ex: SO 3 2- is sulfite SO 4 2- is sufate
Presence of hydrogen indicated by using hydrogen. Prefixes are used to indicate how many hydrogen › Ex: H 2 PO 4 2- : dihydrogen phosphate. MUST KNOW: CO 3 2-, OH -, NO 3 -, NO 2 -, phosphate, sulfate, sulfite.
K 2 CO 3 Name cation: name of the element. Name anion: what is the charge? Write it out Potassium carbonate