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Unit 2 Test-Dr. Herr

Chemistry, Dr. Herr, physical science

QuestionAnswer
subatomic particles: proton, neutron, electron positive, neutral, negative charges
atomic number number of protons
atomic mass number of protons+neutrons
isotopes same # protons, different number neutrons
valence electrons when n=1 max of 2 s electrons
valence electrons when n=2 3 possible pairs of electrons ("p" level)
outer level of electrons never more than 8
periodic table came from Mendeleev elements arranged in in increasing atomic #
Chemical families I. alkali metals II. alkali earths B. Transition elements VII. Halogens VIII. Nobel gases
metals give up electrons they become positive (cations)
nonmetals take electrons they become negative (anions)
ionic bonds formed when oppositely charged ions are formed
electronegativity increases towards Fluorine
semi-conductors elements that are at the metal/non-metal border
ionic compounds a cation (metal) and an anion (nonmetal) join from opposite ends of the chart. metal listed first and nonmetal ends w/ -ide
covalent bonds electrons are shared between two elements near each other on chart (usually non-metals)
examples of covalent bonds atmospheric gases, water, organic compounds, and ionic complexes
metallic bonds special sharing of electrons among many molecules of same element
chemical rxns reactants on left → products on right, reaction energy above arrow, indicate phase produced
a MOLE the atomic mass expressed in grams
Acids non-metals combine w/ H and when dissolved in H2O H ions are released
Bases metals combine w/ OH and when dissolved in H2O, OH (hydroxyl) ions are released
pH scale measures the amount of H+ in a solution. neutral water is a 7. <7 is Acid and >7 is Base
Acid/Base reaction both the acid and base are neutralized and form a salt
Created by: courtney_b90
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