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58 Cards in this Set
- Front
- Back
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Matter
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A solid, liquid, or gas
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Solid
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Has definite shape and volume
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Liquids and gases
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fluid matter, takes shape of container
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Gases
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volume changes drastically with changes in temperature and pressure
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Homogenous mixture
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Has uniform density throughout and no distinguishable components (milk)
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Heterogeneous mixture
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Components are readily distinguishable (chicken soup)
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Element
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simple substance represented by a letter of combination
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Compound
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combinations of elements in whole number ratios
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Law of conservation of mass
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states equations must be balanced
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Chemical reaction
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breaking of bonds and reforming of new bonds to create new chemical compounds with different chemical formulas and properties
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Synthesis reaction
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2 elements combine to form a product
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Decomposition reaction
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breaking of a compound into component parts
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Combustion reaction
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reaction of compound or element with oxygen
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Single replacement reaction
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consists of more active metal reacting with an ionic compound containing a less active metal to produce a new compound
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Double replacement reaction
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a positive ion from one compound combines with the negative ion of the other compound. Result is two new ionic compounds that switched partners
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Atomic number
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= number of protons (or neutrons)
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Number of neutrons
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= atomic number - mass number
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Group 1 A
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has +1 charge
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Group 2A
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has + 2 charge
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Group 3A
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has +3 charge
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Group 5A
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Has -3 charge
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Group 6A
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has -2 charge
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Group 7A
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has -1 charge
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Protons
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has positive charge
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Electrons
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have negative charge
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protons and neutrons
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have same mass
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mass number
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= protons + neutrons
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nucleus
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contains protons and neutrons, electrons are located in orbitals
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chemical reactions
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atoms reach stable electron configurations
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nuclear reactions
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takes place in nucleus to obtain stable nuclear configurations
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radioactivity
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the emission of particles from an unstable nucleus
3 types: Alpha, beta and gamma |
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Alpha radiation
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emission of helium ions. 2 protons and 2 neutrons. +2 charge. Particles can be stopped by paper.
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Beta radiation
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product of a decomposing neutron. Negative charged. Particles can be stopped by foil.
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Gamma radiation
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High energy electromagnetic radiation. Has no charge or mass. Particles can be stopped by several feet of concrete or several inches of lead
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Ionic bond
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attraction between 2 oppositely charged ions. Metal + nonmetal
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Single covalent bond
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2 atoms share pair of electrons
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Double covalent bond
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2 electron pairs are shared
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triple covalent bond
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3 electron pairs are shared
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covalent bond
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strongest type of chemical bond. nonmetal + nonmetal
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Nonpolar covalent bond
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electrons are shared equally
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Polar covalent bond
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elements dont share electrons equally
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Polarity
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difference in electronegativity values for the elements in bond. Greater difference, more polar bond
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Intermolecular forces
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Hydrogen bonding, dipole interactions and dispersion forces.
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Hydrogen bond
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attraction for a hydrogen atom by a highly electronegative element. (Fluorine, chlorine, oxygen, nitrogen) Strongest of intermolecular forces.
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Dipole interactions
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attractions of one dipole for another. Weak intermolecular force
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Dipole
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created when electron pair in a covalent bond is shared unequally resulting in a bond with the more highly electronegative element is slightly negative and the less is slightly positive.
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Dispersion forces
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usually nonpolar covalent. Weakest intermolecular force
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Mole
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amount of substance that contains 6.02 x 10^23 particles.
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atomic mass
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mass of 1 mole of a substance
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stoichiometry
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deals with quantities and numbers between compounds in a chemical equation
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coefficients
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numbers put in front of a compound to be balanced in a chemical equation
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Ways to increase reaction rate
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= increase temp, surface area, concentrations of reactants and add a catalyst
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Redox equation
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oxidation and reduction reactions combined. Reactions involve transfer of electrons from one element to another
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Oxidation
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Loss of electrons
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Reduction
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Gain of electrons
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Oxidation number rules
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1) any elemental atom is 0. (except H, Br, O, N, Cl, I, and F)
2) number of any ion is the charge 3) number for O is -2 4) number for H is +1 5) the sum equals the charge on molecules or polyatomic ions |
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acids
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hydrogen ion donors. pH is less than 7
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bases
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OH-. pH is greater than 7
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