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39 Cards in this Set
- Front
- Back
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Daltons atomic theory of matter
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the basic premise: all matter is made up of extremely small particles called atoms
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Atom
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an extremely small particle of matter the retains its identity during a chemical reaction
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Element
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a type of matter composed of only one kind of atom
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Compound
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a type of matter composed of atoms of 2 or more elements chemically combined in fixed properties
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Chemical reaction
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a process in which one set of substances (reactants) is transformed into another set of substances (products) via rearrangement of atoms
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Atoms of an element are not changed into atoms of a different element by chemical reaction:
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atoms are not created or destroyed during chemical reaction
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Law of constant composition
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in a given compound, the relative number and kinds of atoms are constant
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law of multiple proportions
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if 2 or more elements can combine to form more than one compound, the masses of the element that combined with the fixed mass of the other element are in ratios of small whole numbers
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Law of conservation of mass
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the total mass of materials present after a chemical reaction is the same as the total mass present before the reaction (matter can neither created nor destroyed)
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Atomic structure: Electron
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Mass
9.10939E-31 Charge (C) -1.60218E-19 Charge (e) -1 |
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Atomic structure: proton
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Mass (Kg)
1.67262E-27 Charge (C) +1.60218E-19 Charge (e) +1 |
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Atomic structure: neutron
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Mass (Kg)
1.674493E-27 Charge (C) 0 Charge (e) 0 |
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Nucleus
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P+N
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Atomic # (Z)
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number of protons
-written in subscript |
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Mass # (A)
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P+N
--written in superscript |
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Relative mass
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the mass of an atom in comparison with the mass of another atom
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AMU
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atomic mas unit- a mass exactly equal to 1/12 mass of the carbon-12 atom
1 amu = 1.66054E-24 g 1 g = 6.02214E23 amu |
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Isotope
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same atomic # but different mass #'s
same protons but different # neutrons |
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Atomic weight (mass)
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average mass
weighted average of all the masses of all naturally occuring isotopes |
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Periodic table:
Groups Periods |
Groups -vertical
Periods- horizontal |
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Metalloid
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properties of both metal and non metal
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Characteristics of Metals
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high thermal conductivity
high electrical conductivity metallic luster maleability ductility |
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Chemical bond
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a strong attractive force that exists between certain atoms of ions of a substance
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Ionic bond
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Electrostatic attraction between oppositely charged ions
Results from transfer of electrons Generally formed between metal and non metal |
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Covalent bond
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Attraction between atoms that are sharing a pair of electrons
Results from sharing electrons between atoms Generally formed between non metals |
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______ indicates the exact number of atoms of each element in a molecule of that substance
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Molecular formula
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_______ has subscripts in the smallest possible whole number ratio.
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empirical formula
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Ions car a ___ charge
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net
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Cation
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+
metals tend to lose electrons |
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Anion
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-
non metals tend to gain electrons |
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Oxanions
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oxygen
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Polyatomic ions
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multiple atoms
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Ionic compound
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the empirical formula of an ionic compound represents a formula unit- simplest combining ration of cations and anions
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Formula weight (mass)
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the mass in amu of the one formula unit
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molecular substance
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existis as molecules
formula represents a molecule mass is given as molecular weight (mass) -only non metals |
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Ionic compounds
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exist as ions
formula represents formula unit mass is given as formula weight (mass) -metals and non metals |
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Acids
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molecular compound that dissolves in water to form protons (H+)
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Binary acid
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2 elements
hydrogen plus element |
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Oxoacid
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dissolves ... unfinished card
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