Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
92 Cards in this Set
- Front
- Back
Chemistry is the study of ______ and the changes that it undergoes
|
matter
|
|
______ is anything that has mass and taks up space.
|
Matter
|
|
Each _______ is made up of the same kind of atom.
|
element
|
|
A ________ is made up of two or more different kinds of elements.
|
compound
|
|
The three states of matter are _____, ______, and ___.
|
solid, liquid, gas
|
|
A ___________ mixture is not uniform throughout.
|
heterogeneous
|
|
An example of a ________ property is its boiling point.
|
physical
|
|
________ properties can only be observed when a substance is changed into another substance.
|
Chemical
|
|
The SI units of temperature are expressed in degrees ______.
|
Kelvin
|
|
The term __________ ______ refers to digits that were actually measured.
|
Significant digits
|
|
The smallest particle of matter is the ____.
|
atom
|
|
Atoms are neither _______ nor _________ in chemical reactions.
|
created destroyed
|
|
_________ are formed when atoms of more than one element combine.
|
compounds
|
|
The elemental ___________ of a pure substance never varies.
|
composition
|
|
The law of concervation of mass states that the mass of substance present at the end of a chemical process is _____ to the mass of subtances present before the reaction took place.
|
equal
|
|
The charge on an electron is a ________ ___.
|
negative one
|
|
The charge on a proton is a ________ ___
|
positive one
|
|
A _______ has a mass of one amu and is neutral
|
neutron
|
|
_____________ is the spontaneous emission of radiation by an atom
|
radioactivity
|
|
Protons and neutrons are located in the _______ of an atom.
|
nucleus
|
|
The mass of an atom is calculated by adding thenumber of _______ to the number of ________.
|
protons, neutrons
|
|
12/6 C, the 6 in the symbol represents the ____ ______
|
atomic number
|
|
Atoms of the same element with different masses are called ________ and only differ by the number of ________
|
isotopes, neutrons
|
|
The ________ ______ is a systematic catalog of the elements which are arranged in the order of their ______ ________
|
periodic table, atomic numbers
|
|
_________ formulas give the lowest whole-number ratio of atoms of each element in a compound while _________ formulas give the exact number of atoms of each element in a compound.
|
Empirical, molecular
|
|
Name two different types of reactions.
|
combustion reaction, decomposition reaction
|
|
The sum of the atomic weights of the atoms in a molecule is called the ________ ______.
|
molecular weight
|
|
C6H12o6 = . CO2 =6 H20. The underlined 6 is called the ___________.
|
coefficient
|
|
The units of molar mass are _____ ____.
|
grams per mole
|
|
What is the definition of energy?
|
The capacity to do work or produce heat.
|
|
When energy is used to cause an object that has mass to move, it is called ____.
|
work
|
|
What is the definition of heat?
|
The energy used to cause the temperature of an object to increase.
|
|
Distinguish between PE and KE.
|
PE is inergy of position, KE is energy of movement
|
|
The formula for KE is
|
1/2MV2
|
|
The SI unit of energy is the _____.
|
Joule
|
|
One J is equal to
|
1kgm2/sec2
|
|
An older non-SI unit still used is the _______, which is equal to _____J.
|
calorie, 4.184J
|
|
The formula for work is ________explain each symbol.
|
W=F*D
w=work f=force d=distance |
|
Heat flows from ____ objects to ____ objects.
|
warm cold
|
|
What is the first law of thermodynamics?
|
Energy cannot be created nor destroyed.
|
|
The ________ ______ of a system is the sum of all kinetic and potentiol energies of all components of the system. Its symbol is _____.
|
internal energy, E
|
|
When heat is absorbed by the system from the surroundings the process is __________.
|
endothermic
|
|
When heat is released by the system to the surroundings the process is __________.
|
exothermic
|
|
The internal energy of a system is independent of the path by which the system achieved that state, it is therefore known as a _____ ________.
|
state function
|
|
The thing that students hate to do is called ____. It can be expressed in terms of pressure and volume by the equation ________
|
W=-P(delta)V
|
|
If a reaction is exothermic, its Delta H is always ________.
|
positive
|
|
If a reaction is endothermic, the Delta H is always ________.
|
negative
|
|
The experimental science for measuring the flow of heat is known as ___________.
|
calorimetry
|
|
The amount of energy required to raise the temperature of a substance by 1K is its ____ ________.
|
heat capacity
|
|
_______ law states that as a reaction is carried out in a series of steps, delta H for the overall reaction will be equal to the sum of the enthalpy changs for the individual steps.
|
Hess's
|
|
Standard enthalpies of fomation delta Hf are measured under standard conditions which are _____ degrees and ______ pressure.
|
298K 25C, atmospheric 1STM
|
|
Name three different types of reactions.
|
combustion, neutralization, decomposition
|
|
The sum of the atomic weights of the atoms in a molecule is called the _________ ______.
|
molecular weight
|
|
In a chemical reaction, if there is more of one reactant than is necessary, that reactant is said to be __ ______. The other reactant is known as the _________ _______ and is used in all molar calculations.
|
in excess, limiting reagent
|
|
Solutions are ____________ mixtures of two or more pure substances.
|
homogeneous
|
|
the dissolving medium is called the ________ while the cvhamical dissolved is known as the ______.
|
solvent, solute
|
|
____________ occurs when an ionic substance dissolves in water.
|
Dissociation
|
|
Give five examples of strong acids.
|
HCL, HBR,HI,HNO3,H2SO4,HCLO3,HCLO4
|
|
Give four examples of strong bases.
|
LiOH, NaOH, KOH, Ca(OH)2
|
|
If ions are mixed and react to form an insoluble species, that compound is called a ___________.
|
precipitate
|
|
Metathesis is simply an ________ reaction.
|
exchange
|
|
In an ionic reaction equation the things that don't change are called the _________ ____.
|
spectator ions
|
|
Both definitions of acis involve the ______ _____ or _______.
|
proton donor H+ ion
|
|
Substances that increase the concentration of OH ions are called _____.
|
bases
|
|
The products of the reaction of an acid and a base are always a ____ and _____.
|
salt, water.
|
|
Oxidation is when an atom or ion _____ electrons while recuction is when an atom or ion _____ electrons.
|
loses, gains
|
|
The oxidation state of an element from the periodic table is always ____.
|
zero
|
|
The sum of the oxidation numbers in a neutral compound is equal to ____.
|
zero
|
|
Write the equation for molarity.
|
M= moles of solvent
--------------- volume of solution in liters |
|
Two important properties of waves are their __________ and ________ (words and symbols).
|
wavelength , frequency
λν |
|
The equation for the speed of light is _____________--which is equal to _________
|
c=wavelength*frequency, c=hv, 3.00*10/8 m/s
|
|
Waves do not explain all the properties of light and Max Planck explained this by assuming that energy comes in ______ called ______.
|
packets quanta
|
|
Einstein concluded that energy is proportional to ________, the equation being E=hv.
|
frequency
|
|
h is equal to _______ constant which numerically is _________.
|
Planck
s, 6.63*10-34J-s |
|
Neils Bohr is credited with the theory of ______ ________.
|
atomic orbitals
|
|
Energy is only absorbed or emitted in such a way as to move an electron from one allowed energy state to another, the energy is difined by _________ (equation)
|
E=hv
|
|
de Broglie demonstrated that the relationship between mass and wavelength was ____________(equation).
|
wavelength=h/ mv
|
|
Erwin Schrodinger developed a mathematical treatment that took into account both the wave and particle nature of matter which became known as_______ _________.
|
quantum mechanics
|
|
An orbital is decribed by a set of quantum numbers. Theste quantum numbers are the ______ _______ _____ abbv. _, the _________ _______ ______ abb, L, the ________ _______ ______ abbv __, and finally the ____ _______ ______ abbv. __
|
principal quantum number, n
azimutal quantum number, l magnetic quantum number, ml spin quantum number, ms |
|
For a one electron hydrogen atom, orbitals on the same energy level have the same energy, that is , they are, _________.
|
degenerate.
|
|
No two electrons in the same atom can have exactly the same energy, this is known as the_____ _________ _________.
|
Pauli exclusion principle
|
|
4p5: 4 stands for the ___________, p stands for the _______ and 5 stands for the _________.
|
energy level, orbital, number of electrons in orbital
|
|
For degenerate orbitals, the lowest energy is attained when the number of electrons with the same spin is _________. This is known as ______ ____.
|
maximized, Hundt's rule
|
|
I have told you that I will never give you any exceptions to the rule which your book calls_________.
|
anomalies
|
|
Dmitri Mendeleev and Lathar Meyer were both given credit for creating the ________ _____.
|
periodic table
|
|
Three trends that can be observed using the table are _____ __ _____ ___ ____, _________ _____, _______ ________.
|
sizes of atoms and ions, ionization energy, electron affinity
|
|
The nuclear charge that an electron experiances depends on the following two factors:
|
Electrons are both attracted by the nucleus and repelled by other electrons.
|
|
The effective nuclear charge Zeff is equal to Z-S, where Z is the _____ ______ and S is a ________ _______.
|
atomic number, screening constant.
|
|
The bonding atomic radius is defined as ____ of the distance between __________ bonded nuclei.
|
half, covalently
|
|
Cations are _______ than their parent atoms because the outermost electron is ________ and __________ are reduced.
|
smaller, removed, repulsions
|
|
Anions are ______ than their parent atom because electrons are _____ and __________ are increased.
|
larger, added, repulsions
|
|
What is the definition of ionization energy?
|
The energy required to remove an electron from the ground state of a gaseous atom.
|