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;
113 Cards in this Set
- Front
- Back
The mass that enters into a chemical reaction remains unchanged.
|
Boyle's law
The law of conservation of mass |
|
Mass is neither created nor destroyed in a chemical reaction.
|
The law of conservation of mass
|
|
The elements that compose a compound are present in fixed and precise proportion by mass.
|
The law of constant composition.
|
|
When the same elements can form 2 different compounds, the ratio of masses of one of the elements in the 2 compounds is a small whole number relative to the given mass of the other element.
|
The law of multiple proportions
|
|
States that all atoms of an element were identical and they have the same mass.
|
Dalton's atomic theory
|
|
states elements consisted of tiny particles called atoms. Compounds consisted of atoms of different elements combined together. Chemical reactions involved the rearrangement of combinations of those atoms.
|
Atomic Theory
|
|
a tabular representation of all the elements arranged according to their atomic number (the number of protons in their nucleus) and their chemical properties
|
The periodic table
|
|
The mass of an atom is...
|
the sum of its protons and neutrons.
|
|
What is an isotope?
|
The number of protons for a given element is fixed, but the number of neutrons may vary.
|
|
Where is the atomic number found? the atomic mass?
|
The atomic number is on the top of the element listed on the periodic table. The atomic mass is found under the element.
|
|
What determines the atomic mass?
|
based on the sum of protons & neutrons
|
|
Isotopes change the ______ but not the _______.
|
atomic weight; atomic number
|
|
In the periodic table, columns of elements have what in common?
|
They are elements with similar numbers and characteristics of electrons in the outer orbitals and therefore, similar chemical properties.
|
|
The chemical properties of an element are related to what?
|
Chemical properties are related to the number and characteristics of the electrons in theoutermost (most energetic) orbitals-valence electrons
|
|
The number of electrons is the same as what?
|
the number of protons (the atomic number)
|
|
On the periodic table, what structures are the most stable and why?
|
noble gases are the most stable because they have 8 valence electrons in the outer shell
|
|
On the periodic table what changes in a row when you go from left to right?
|
When you go from left to right on a particular row, the number of valence electrons increases by 1.
|
|
What are valence electrons? what is their significance?
|
electrons that are in the outermost shell. they determine the chemical behavior of an atom
|
|
Atomic size is determined by...
|
how much space the elecrons take up.
|
|
Ionization energy is ...
|
the energy required to remove the outermost electron from an atom.
|
|
ability of an atom to attract electrons.
|
electronegativity
|
|
results from sharing one or more electron pairs between two atoms
|
covalent bonding
|
|
results from electrostatic attractions among ions, which are formed by the transfer of one or more electrons from one atom to another.
|
ionic bonding
|
|
nonmetal to nonmetal bonding
|
covalent bond
|
|
consists of two or more atoms held together by covalent bonds
|
molecule
|
|
the sharing of one pair of valence electrons
|
single bond
|
|
the sharing of two pairs of valence electrons
|
double bond
double bonds put rotation restrictions on molecules |
|
The more bonds the more energy required to break them apart. T/F
|
True
|
|
The more _____ an atom the stronger it pulls shared electrons toward itself.
|
electronegative
|
|
electronegativity _____ from left to right across the periodic table.
|
increases
|
|
The type of bond that shares the electron equally and the atoms have similar electronegativities.
|
nonpolar covalent bond
|
|
The type of bond that share the electrons unequally and the atoms have differing electronegativities.
|
polar covalent bond
|
|
An anion is ...
|
negatively charged (aquired an electron)
|
|
A cation is ...
|
positively charged (gave up an electron)
|
|
What are ions?
|
Charged atoms with more or fewer electrons than usual.
|
|
an attraction between anions and cations
|
ionic bond
|
|
metal bonded with nonmetal
|
ionic bond
|
|
ionic compounds are often called what?
|
salts
|
|
In a solution, each ion is surrounded by ?
|
water molecules
|
|
Negatively charged polyatomic ions have ____ electrons in their covalent bonds than they do protons in all their collective nuclei.
|
more
|
|
Positively charged polyatomic ions have ____ electrons in their covalent bonds than protons in all their collective nuclei.
|
fewer
|
|
Polyatomic ions associate with _______ to produce electrical neutrality in the compound.
|
ions of the opposite charge
|
|
The ____ of the molecule is very important to its function in the living cell and is determined by the positions of its atoms valence orbitals.
|
shape
|
|
determines how biological molecles, recognize and respond to one another with specificity.
|
Molecular shape
|
|
statement of the ratios of elements that make up a compound.
|
formula
|
|
Formula weight is ...
|
the sum of the atomic weights of the constituent atoms of the formula.
|
|
In ___ compounds, the ratio may reflect the actual composition of a molecule.
|
covalent
|
|
In ___ compounds, it is the ratio of ions that make up the compound.
|
ionic
|
|
A mole =
|
6.022 x 10exp23
Avagadro's number |
|
mass in grams numberically equal to the atomic weight of the element in grams
|
molar mass
|
|
1 M solution is...
|
the concentration of one mole of a compound in 1 liter of solution.
|
|
1 M solution could also be 1/10 the formula weight dissolved in
|
100 ml of solution
|
|
Mixtures in which the solvent and solute are intimately associated as molecules or ions
|
Solutions
|
|
Solutions in which the solvent is water
|
Aqueous solutions
|
|
Solutes in aqueous solutions can be ...
|
gases, other liquids, or solids.
|
|
Water molecules are...
|
polar
|
|
Solutes that can interact with the positive or negative (or both) ends of the ater molecule will be...
|
soluble in water.
|
|
Substances that are easily soluble in water
|
hydrophilic
|
|
Substances that are poorly soluble in water
|
hydrophobic
|
|
Hydrophilic/soluble substances are usually...
|
polar
|
|
Hydrophobic/insoluable substances are usually...
|
nonpolar (no charge)
|
|
Solids that dissolve in water are ____ soluble the higher the temperature of the water.
|
more
|
|
Liquids that dissolve in water are...
|
miscible
|
|
Liquids that don't dissolve in water are...
|
immiscible
|
|
Gases dissolve in water because ....
|
they exert pressure on the surface of the water.
|
|
Gases dissolve in water according to their...
|
partial pressure in the atmosphere above/in contact with the water.
|
|
O2 is _____ soluble in water.
|
not very
|
|
CO2 is ____ soluble in water.
|
very
|
|
property that enables substances to become evenly distributed in a solution.
|
Diffusion
|
|
All molecules, ions, and atoms possess ....
|
thermal energy (at temperatures above absolute zero).
|
|
Atoms/molecules/ions in a _______ or in solution are free to move in a straight line until they collide with something.
|
liquid or gaseous state
|
|
Atoms/molecules/ions in a ____ are held in place by strong attractive forces and just vibrate because of their thermal energy.
|
solid
|
|
Substances always diffuse ...
|
down their concentration gradient (from more concentrated areas to less concentrated areas until all areas have equal concentration)
|
|
At equal concentration, _____ movement occurs.
|
no net movement, although individual atoms/molecules/ions are still moving about as they did before.
|
|
basically diffusion that occurs across a semipermeable membrane
|
Osmosis
|
|
The molecules leaving a given area are balanced by the ones arriving in that area. T/F
|
true. remain in a state of equillibrium
|
|
Membrane that will let some of the components of the solution cross but will exclude others.
|
semipermeable membrane
|
|
Most membranes are freely permeable to
|
water.
|
|
lipid membranes that are impermeable to charged molecules
|
cell membranes
|
|
Biological membranes are made of lipids, so most ______ cannot cross.
|
charged substances, such as ions and polar molecules
|
|
If there are concentration differences across biological membranes, _____ must cross the membranes to equalize them.
|
water
|
|
The propensity of water to cross a semipermeable membrane to equalize solute concentrations on either side
|
osmotic pressure
|
|
energy supplying reaction
|
exothermic (reactants are at a higher energy level than the product-energy is produced)
|
|
energy requiring reaction
|
endothermic (energy must be introduced to get the reaction started)
|
|
Increasing the concentration of the reactants_____ the reaction.
|
speeds up
|
|
Increasing the temperature ____ the reaction.
|
speeds up
|
|
speed up reactions by lowering the activation energy
|
catalysts
|
|
Catalysts ____ entropy, which is a measure of _______ that contributes to the activation energy.
|
reduce; randomness
catalysts speed up reactions by making productive collisions between the reactants more likely |
|
Catalysts are usually...
|
protein molecules called enzymes.
|
|
Enzymes reduce the _____ by reducing the ______.
|
activation energy; entropy
|
|
Many chemical reactions are ...
|
reversible-they go forward or backward.
|
|
Reversible reactions can go completely forward or completely backward. T/F
|
False. Reactions will never go completely forward or completely backward.
|
|
Reversible reactions have an ______ between the forward and the backward reaction.
|
equillibrium
|
|
States any change in status quo prompts an opposing reaction in the responding system.
|
The Principle of LeChatelier
|
|
When the concentration of one of the reactants is increased, the reaction is pushed toward the
|
right
|
|
When the concentration of one of the products is increased, the reaction is pushed to the
|
left
|
|
Some isotopes of elements with atomic numbers less than or equal to 83 and all elements with atomic numbers greater than 83 are...
|
radioactive
|
|
Isotopes that have nuclei that are unstable and emit energy in the form of particles or electromagnetic waves
|
radioactive
|
|
2 protons and 2 neutrons (a helium nucleus) emitted as a group
|
alpha particle
|
|
electron that comes from the nucleus
|
beta particle
|
|
a high energy electromagnetic wave, of higher energy than x-rays
|
gamma ray
|
|
particle the size of an electron but with a positive charge
|
positron
|
|
When alpha or beta particles are emitted what happens?
|
the nucleus changes its atomic number (number of protons) and hence becomes another element
|
|
Radioactive elements decay according to a ____ which is different for each element and isotope.
|
half life
|
|
Isotopes in nuclear medicine, have ____ half lives.
|
extremely short; good to have a short life for radioactive isotopes because after the scan is done, the radioactivity rapidly disappears
|
|
Isotopes used in radiation medicine have ____ half lives.
|
longer; days, weeks, or in some instances, years
|
|
Patients given a radioactive isotope by IV will have radioactive excreta. T/F
|
True; must be handled per protocol
|
|
If the patient has a radioactive implant, their excreta will be radioactive. T/F
|
False. The excreta is not radioactive because it is confined by the sealed implant.
|
|
Radioactivity produces ____ of chemicals that it hits.
|
ionization
|
|
In the case of human exposure, the most damaging ionization occurs in ...
|
the person's DNA.
Ionizing radiation can produce so much DNA damage that the cell dies. This is the purpose of ionizing radiation directed at tumors. |
|
Ionizing radiation may produce smaller amounts of DNA damage that survive as ...
|
permanent mutations.
|
|
Mutations may combine with other mutations in the same cell to produce
|
malignant transformation
|
|
Patients who have received radiation to treat one cancer have increased their chances of what?
|
increased incidence of second malignancy in the area that they received radiation
|