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102 Cards in this Set
- Front
- Back
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What is Matter
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Anything that has mass and takes up space (has volume)
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What is the difference between Mass and Weight?
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Mass measures the of amount of matter while, Weight measures the pull of gravity on matter.
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Chemical Change
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Matter changes its identity
EX. Log on fire -Old substances used up and new ones formed |
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Physical Change
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Matter keeps its identity
EX.Salt in water -Dissolving substance or changing state (phase) between solid, liquid and gas |
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1 in is equal to how many cm?
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2.54 cm
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1lb is equal to how many grams?
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453.6g
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1qt iis equal to how many L?
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0.946L
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Conversion from Fahrenheit to Celsius.
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Degree Celsius= 5/9(Fahrenheit-32)
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Conversion from Celsius to Fahrenheit.
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Degree fahrenheit=9/5Degree Celsius +32
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Conversion to Kelvin
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Degree Celsius+273
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How many cm in 1 inch
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2.54cm
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How many grams in 1 lb
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453.6g
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Formula for Density
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Density=Mass/Volume
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The Law of Conservation
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Energy cannot be created or destroyed.
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1kcal=how many Calories?
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1000 cal
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1 cal= how many Joules
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4.184J
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What is Specific Heat?
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The amount of heat change when matter is heated or cooled
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The Equation for Specific Heat is?
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Amount of Heat=Specific Heat x mass x change in temperature.
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Pure Substances
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fixed composition; cannot be further purified
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What is a Monotomic Element?
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Exists as single atoms
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Diatomic Elements
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Occur as diatomic molecules (pairs of atoms)
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Polyatomic Emelments
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Have three or more atoms per molecules
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Compound
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Pure substance made up of two or more elements in a fixed ratio by mass
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Mixture
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Combination of two or more pure substances
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Heterogeneous mixture
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Substances are not evenly distributed throughout
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Homogeneous Mixture
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Substances are evenly distributed throughout.
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Daltons Atomic Theory
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All matter is composed of very tiny particles (atoms). A molecule is a tightly bound combination of two or more atoms that acts as a unit
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Law of Conservation Mass
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Mass can be neither created or destroyed
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Law of Constant Composition
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Compounds have a definite composition by mass
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Subatomic Particles
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The unit of mass is the atomic mass unit (amu)
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What is a AMU
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one amu is defined as one-twelfth the mass of an atom of carbon with 6 protons and 6 neutrons in its nucleus
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Mass Number
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Sum of the number of protons plus neutrons in the nucleus of an atom
(Top Number) |
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Atomic Number
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Number of protons in the nucleus of an atom
(Bottom Number) |
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Isotopes
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atoms with the same number of protons but a different number of neutrons
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Atomic Weight
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weighted average of masses of isotopes of an element
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Metals
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Solids (except Hg), shiny, conduct electricity, ductile, and malleable
Tend to give up electrons to form positive ions |
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Nonmetals
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On right side of Periodic Table (except H)
Brittle, dull, poor conductors of electricity Tend to accept electrons to form negative ions |
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Mettalloids
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B, Si, Ge, As, Sb, Te
Have some properties of metals and some of nonmetals Silicon is a semiconductor Does not conduct electricity at low voltages, but becomes a conductor at higher voltages |
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Electrons: Ground state vs. excited
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Ground state: the electron configuration of lowest energy while,
Excited state: Electron has more than lowest possible energy |
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Electron Distribution
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electrons are distributed into shells around the nucleus
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Principal Energy Level (Shells)
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has different maximum number of electrons it can hold. They are subdivided into orbitals
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Orbitals
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Each orbital can hold up to 2 electrons. Each Orbital has a different energy, the lowest energys fill first
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Electron Configuration
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Rule 1: Lowest energy orbitals fill first
Rule 2: Each orbital can hold a maximum of two electrons (with opposite spins) Rule 3: Orbitals of equal energy each add one electron first, then add second electron to fill them completely. |
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Orbital Box Diagram
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a box represents an orbital
an arrow represents an electron a pair of arrows with heads in opposite directions represents a pair of electrons with paired spins |
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Ionization Energy
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the energy required to remove the most loosely held electron from an atom in the gaseous state
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Valance vs. Core Electrons
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Valance Electrons are the elecrons in the Valance shell, while the Core Electrons are the electrons in the outermost shell
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Anion vs Cation
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Anions are Negative ions formed when an atom gains electrons while, cations are Positive ions formed when an atom loses electrons
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Ionic Bonds
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the force of electrostatic attraction between a cation and an anion
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Covalent Bond
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a pair of electrons that are shared by two atoms
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Electronegativity
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measure of an atom’s attraction for shared pair of electrons in chemical bond with another atom
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Polarity (Polar Vs NonPolar)
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Nonpolar: Electrons are shared equally
Polar: Electrons are NOT shared equally |
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Bonding electrons vs Nonbonding electrons
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Bonding (shared) electrons are shown as bonds (lines)
Nonbonding electrons are represented as a pair of Lewis dots |
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Types of bonding
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single bond, atoms share one pair of electrons; in a double bond, they share two pairs, and in a triple bond they share three pairs
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Reactants and Products
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in a chemical reaction one or more reactants is converted to one or more products
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Formula Weight
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the sum of the atomic weights in atomic mass units (amu) of all atoms in a compound’s formula
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Molecular Weight
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Molecular compounds only
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What is a Mole
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amount of substance whose mass in grams is numerically equal to its molecular or formula weight
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What is Avogadro's Number
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Number of formula units in a mole
6.02214199 x 1023 formula units per mole |
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Molar Mass
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the formula weight of a substance expressed in grams
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Stoichiometry
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the study of mass relationships in chemical reactions
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Limiting reagant
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the reagent that is used up first in a chemical reaction
-Need to determine which reagent is present with the fewest moles |
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Actual Yield
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the mass of product formed in a chemical reaction
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Theoretical Yield
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the mass of product that should be formed according to the stoichiometry of the balanced chemical equation
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Percentage Yield
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actual yield divided by theoretical yield times 100
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Reactions Occur when?
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a precipitate (solid) forms (see solubility table)
a compound that is insoluble in water a gas is formed (bubbles or fizzing) an acid neutralizes a base and water is formed one of the ions can oxidize another (Redox reaction) |
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Oxidation-reduction (redox) reaction
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any reaction in which electrons are transferred from one species to another
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Exothermic vs Endothermic
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Endo Heat absorbed, exo Heat given off
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Kinetic Molecular Theory of Gases
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Gas particles have negligible volume compared to volume gas occupies
Particles move through space in straight lines Kinetic energy (KE) proportional to temperature (K) Can collide with container or each other Total KE before collision = KE after collision Collisions with walls of container exert pressure |
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Pressure Units
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1atm= 760mmhg
=760 torr |
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Boyles Law
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Volume and pressure are inversely proportional (fixed mass and gas at a constant temperature
P1V1=P2V2 |
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Charles Law
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Temperature and volume are directly proportional (fixed mass and pressure); Temperature is in kelvins (K)
V1/T1=V2/T2 |
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Gay-Lussac's Law
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Pressure and temperature are directly proportional (fixed mass and volume); Temperature in kelvins (K)
P1/T1=P2/T2 |
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Combined Gas Law
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Boyle’s law, Charles’s law and Gay-Lussac’s law
P1V1/T1=P2V2/T2 |
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Avadagro's Law
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volume of gas is directly proportional to its molar amount at a constant pressure and temperature
V/n=constant |
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Idea Gas Law
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Can be used for a single sample that does not change
PV=nRT |
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Daltons Law of Partial Pressure
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the total pressure, PT, of a mixture of gases is the sum of the partial pressures of each individual gas
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London Dispersion Forces
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the attraction between very temporary induced dipoles
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Dipole-dipole interactions
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The electrostatic attraction between positive and negative dipoles
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Hydrogen Bonds
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a hydrogen covalently bonded to an atom of high electronegativity (O, N, F) is attracted to another O, N or F
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Solutions are composed of what?
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Solutes: substance that is dissolved
Solvent: substance that the solutes are dissolved in |
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The difference between Saturated, Unsaturated and Supersaturated.
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Saturated: Maximum amount of solute
Unsaturated: Less solute than saturated Supersaturated: More solute than saturated (unstable) |
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Henry's Law
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the solubility (or concentration) of a gas in a liquid is directly proportional to the partial pressure of the gas over the liquid
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Equation for molarity
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Molarity(M)=moles of solute(n)/Liters of solution(L)
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Strong vs weak electrolytes
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Strong electrolyte: a compound that dissociates completely in an aqueous solution
Weak electrolyte: a compound that only partially dissociates in an aqueous solution |
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Water as a Solvent
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Polar covalent molecules dissolve because they are solvated by hydrogen bonding
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Colloid
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a solution in which the solute particle diameter is between 1nm and 1000 nm
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Osmolarity
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the molarity multiplied by the number of particles produced by each formula unit of solute
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Dialysis
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the separation of larger molecules, dissolved substances, or colloidal particles from smaller molecules, substances, or colloidal particles by a semipermeable membrane
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Chemical Kinetics
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the study of the rates of chemical reactions
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what effects the rate of a reaction?
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Molecular collisions
Activation energy Nature of the reactants Concentration of the reactants Temperature Presence of a catalyst |
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effective collision
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a collision that does not result in a reaction
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activation energy
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the minimum energy required for a reaction to take place
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Catalyst
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a substance that increases the rate of a chemical reaction without itself being used up
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Equilibrium
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a dynamic state in which the rate of the forward reaction is equal to the rate of the reverse reaction
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Le Chatelier's Principle
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when a stress is applied to a chemical system at equilibrium, the position of the equilibrium shifts in the direction to relieve the applied stress
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Strong acid vs a weak acid
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Strong acid: one that reacts completely or almost completely with water to form H3O+ ions
Weak acid: a substance that dissociates only partially in water to produce H3O+ ions |
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Strong Base vs Weak Base
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Strong base: one that reacts completely or almost completely with water to form OH- ions
Weak base: a substance that dissociates only partially in water to produce OH- ions |
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Acid-Base Reaction
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a proton transfer reaction
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Conjugate acid-base pair
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any pair of molecules or ions that can be interconverted by transfer of a proton
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Bronsted-Lowry Definition
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do not require water as a reactant
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Acid-Base Equilibrium
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For weak acids, significant amounts of both the acid and its conjugate base will be present and form an equilibrium
Equilibrium lies on the side of the weaker acid and weaker base. |
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Titration
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Volume of a solution of know concentration is added to a solution ofunknown concentration. Measure amount of known solution needed to react exactly with original material - at endpoint
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