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Chemical Bonds Test

8th Grade NSA

TermDefinition
Covalent bond A bond formed between two nonmetals where they share valence electrons
Valence electrons Electrons in the outermost energy level/shell of an atom that are involved in (chemical) bonding
Double covalent bond A covalent bond where two pairs of electrons are shared
Triple covalent bond A covalent bond where three pairs of electrons are shared
Ionic compound A compound formed between a metal and a nonmetal where electrons are transferred
Covalent compound (or molecular compound) A compound formed between two nonmetals where electrons are shared
Polyatomic ion A charged group of atoms that behaves as a single unit in a compound
Naming steps for ionic compounds Write the name of the metal (or positive ion) first and leave it unchanged. Write the name of the nonmetal and replace the last syllable with "ide".
Naming steps for covalent compounds Write the name of the first nonmetal and leave the ending unchanged. Write the name of the nonmetal and replace the last syllable with "ide". If there are more than one nonmetal, add a (Greek) prefix in front of each nonmetal.
Naming steps for polyatomic ionic compounds Write the name of the metal (or positive ion) first and leave it unchanged. Write the unique name of the polyatomic ion and leave it unchanged.
Covalent compounds general properties - Huge variety of compounds - Soft if solids - Low melting points - Electrical insulators - Do not dissolve well
Examples of covalent compounds - Stomach acid (HCI) - Natural gas (CH4) - Table sugar (C12H22011) - Rubbing alcohol (C3H80)
Common polyatomic ions - NH4+ = ammonium - OH- = hydroxide - CO3 2- = carbonate - NO3- = nitrate - CN- = cyanide - MnO4- = permanganate - HCO3- = hydrogen carbonate - CrO4 2- = chromate - Cr2O7 2- = dichromate - SO4 2- = sulfate - PO4 3- = phosphate
Examples of polyatomic ionic compounds - NaOH = sodium hydroxide - K2CO3 = potassium carbonate - NH4NO3 = ammonium nitrate - Ca(OH)2 = calcium hydroxide - MgSO4 = magnesium sulfate
Examples of covalent compounds - H2O = water - CO2 = carbon dioxide - CH3OH = methanol - C6H12O6 = glucose - CCl4 = carbon tetrachloride
Examples of ionic compounds - NaCl = sodium chloride - MgO = magnesium oxide - Al2O3 = aluminum oxide - CaCO3 = calcium carbonate - FeCl3 = iron(III) chloride
Chemical bond is formed when two or more different elements chemically combine together.
Noble gases do not form compounds naturally because their outer electron shell is full.
Ionic bonding What happens- gaining or losing electrons.
Covalent bonding What happens- sharing electrons.
Valence electrons are the electrons found in the outermost energy level, or shell, and they participate in chemical bonding.
Valency/Valence number The number of outer energy level electrons in an element is also called its
Ion is an atom that has a positive (+) or negative (-) charge.
Ionic bond is formed due to the attraction between (+) and (-) ions.
Ionic bonds form between a metal and a nonmetal.
During the formation of an ionic bond, the metal loses valence electrons while the nonmetal gains valence electrons.
Ionic compounds form -crystals -hard and brittle - have very high melting points - conductors when dissolved in water -insulators when solid
Examples of ionic compounds -plant fertilizer (KN) -tooth fluoride (NaF) -M&M logo (TiO2) - bone minerals (CaO).
In their natural state atoms have no overall charge. This is because in the nucleus, the number of __________ equals the number of __________. protons (+) electrons (-)
Created by: user-1806441
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