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44 Cards in this Set
- Front
- Back
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Precision
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number of significant figures or uncertainty
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Percent error
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expresses the relative accuracy of a measurement
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Scientific notation
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allows us to write a number in an easy-to-read manner/between 1 and 10 multiplied and raised to an exponent
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Atom
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the smallest unique particle that characterizes an element
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Electrostatic forces
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attract protons and electrons to each other
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Isotopes
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atoms of the same element with different mass numbers
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Atomic mass
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an element’s weighted average of all of the naturally occurring isotopes found in nature
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Structural formulas
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each compound has a unique arrangement of atoms in the molecular unit
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Formula unit
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the formula of an ionic compound shows the type and number of ions
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Physical properties
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undergo physical changes (physical state can change due to changes in temperature like melting point of a solid (or freezing point), boiling point (or condensation point)
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Chemical changes
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observe the law of conservation of mass
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Density
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relates to the mass of a substance to its volume
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Extensive properties
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mass and volume (vary)
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Intensive properties
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independent from the amount present
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Heterogeneous mixtures
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can be separated by filtration
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Homogeneous mixture
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a solution with one phase, can be separated by distillation
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Avogadro’s number
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6.022E23
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Single-replacement reactions
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a metal exchanges places with the cation of a different metal
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Double-replacement reactions
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involve the exchange of ions between two soluble compounds
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Stoichiometry
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in these problems the balanced equation provides the mole ratios for conversion from moles to another compound in the reaction to moles of another
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Limiting reactant
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completely consumed; it determines the amount of product formed
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Percent yield
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actual yield/theoretical yield
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Wave mechanics
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takes into account the wave nature of the electron
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Orbital
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the electron is viewed as having a certain probability of existing in a region of space
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Shells
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principal energy levels
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Subshell
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the orbitals of one type within a particular shell make up a…
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Ionic bonds
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the ions formed by the electron exchange are arranged in a lattice structure which are held together by…
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Covalent bonds
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two nonmetals follow the octet rule by electron sharing
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Polar covalent
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when electrons are not shared equally and contains a dipole
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Non polar covalent
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atoms of the same element share electrons equally
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Polar
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if the bond dipoles are not the same in each direction or they do not cancel
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Dispersion forces
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occur between all molecules but act exclusively for nonpolar molecules
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Dipole-dipole force
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if a molecule has a permanent dipole
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Hydrogen bonding
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involves hydrogen bonded to an F, O, N interacting with an electron pair on an F, O, N on another molecule
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Ionic compounds
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dissolve in water because the ion-water forces
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Polar covalent molecular compounds
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dissolve in water as discrete molecular, or they may undergo ionization
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Colligative properties
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vapor pressure lowering, boiling point elevation, freezing point loweringosmotic pressure elevation (process of osmosis)
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Oxidized
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the reactant that gives up or loses electrons
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Reduced
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reactant that gains the electrons
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Reducing agent
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reactant oxidized
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Oxidizing agent
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reactant reduced
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Rate of RXN
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Frequency of collisions & activation energy: the magnitude of the activation energy/the temperature/the concentration of reactants/the particle size in heterogeneous mixtures/a catalyst
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Le Chatelier’s Principle
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the factors that can shift the point of equilibrium/concentration, pressure, temperature
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Types of radiation
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alpha particles, beta particles, and gamma rays
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