Chapter 2 Vocab Flashcards
Inorganic Compounds
a simple substance that does not contain a carbon backbone
Organic Compounds
a compound consisting of a backbone made up of carbon atoms
Elements
substances that cannot be broken down into simpler substances by ordinary chemical reactions
Chemical Signal
the abbreviation for an element;usually the 1st letter (or 1st and 2nd letters) of the English or Latin name
Trace Elements
they are only required in minute amounts
Atom
the smallest portion of an element that retains its chemical properties
Matter
anything that has mass and takes up space (subatomic particles)
Nucleus
central region of the atom that contains the protons and neutrons
Atomic Number
the number of protons in the atomic nucleus of an atom, which uniquely identifies the element to which the atom corresponds
Atomic Mass Unit (amu)(dalton)
the approximate mass of a proton or neutron
Atomic Mass
number that indicates approximately how much matter that atom contains compared with another atom (#of protons + # of neutrons)
Radioisotopes
unstable isotopes that spontaneously emit radiation
Isotopes
an alternative form of an element with a different number of neutrons but the same osmotic pressure
Autoradiography
radiation causes the appearance of dark silver grains in photographic film
Orbitals
region in which electrons occur in an atom or molecule
Electron Shell
group of orbitals of electrons with similar energies
Valence Shell
outermost ring in a Bohr model
Valence Electrons
electrons in the outer electron shell, known as the valence shell, of an atom, in the formation of a chemical bond
Molecules
2 or more atoms may become joined ver strongly to form a stable particle
Chemical Formula
shorthand expression that describes the chemical composition of a substance
Simplest Formula (empirical)
a chemical formula that gives the smallest whole-number ratio of the component atoms
Molecular Formula
the type of chemical formula that gives the actual numbers of each type of atom in a molecule
Structural Formula
a type of chemical formula that shows the spatial arrangement of the atoms in a molecule
Avogadro’s Number
the number of units (6.02 e23) present in 1 mole of any substance
Reactants
the substances that participate in the reaction
Products
the substances formed by the reaction
Dynamic Equilibrium
the rates of the forward and reverse reactions are equal
Bond Energy
the energy required to break a particular chemical bond
Covalent Bonds
sharing of electrons beween atoms in a way that results in each atom having a filled valence shell
Covalent Compound
a compound in which atoms are held together by covalent bonds
Orbital Hybridization
a rearrangement of the orbitals in the valence shell that may occur when an atom forms covalent bonds with other atoms
Electronegativity
a measure of an atoms attraction for electrons
Polar Molecule
one end with a partial positive charge and another end with a partial negative charge
Cations
positively charged ions
Anions
negatively charged ions
Ionic Bonds
the chemical attraction between a cation and an anion
Solute
a dissolved substance
Surface Tension
the attraction that the molecules at the surface of a liquid may have for one another
Hyrophilic
substances that interact readily with water
Hydrophobic
water fearing
Hydrophobic interactions
the tendency of hydrophobic substances to cluster together due to strong cohesive interactions among surrounding water molecules
Kinetic Energy
energy of motion
Heat
the total amount of kinetic energy
Temperature
measure of the average kinetic energy
Heat of Vaporization
the amount of heat energy required the change 1g of a substance for the liquid phase to the vapor phase
Calorie
amount of hat energy required to raise the temperature of 1g of water 1 degree celsius
Specific Heat
amount of energy required the raise the temperature of water
Acid
proton donor
Base
proton acceptor
pH
-log10 [H+]
Ionic Compound
a substance consisting of cations and anions, which are attracted by their opposite charges, they do not consist of molecules
Solvent
liquid capable of dissolving many substances
Hydration
process of association of a substance with a partial positive and/or negative charges of water molecules
Hydrogen Bond
a weak attractive force existing between a hydrogen atom with usually oxygen or nitrogen
Van der Walls Interactions
weak attractive forces between atoms; caused by interactions among fluctuating charges
Redox Reaction
the chemical reaction in which 1 or more electrons are transferred from 1 substance (oxidized) to another (reduced)
Oxidation
the loss of 1 or more electrons (hydrogen atoms) by an atom, ion, or molecule
Reduction
the gain of 1 or more electrons (hydrogen atoms) by an atom, ion, or molecule
Cohesion
ring-shaped protein complex responsible for linking siste chromatids during prophase
Adhesion
the property of sticking to some other substance
Capillary Action
the ability of water to move in small-diameter tubes as a consequence of its cohesion and adhesion
Neutral Solution
pH of 7, equal concentrations of hydrogen ions [H+] and hydroxide ions [OH-]
Acidic Solution
hydrogen ions > hydroxide ions; pH <7
Basic Solution
hydrogen ions7
Buffer
resists changes in pH when an acid or base is added
Salt
hydrogen ion of an acid is replaced by some other cation
Electrolytes
a substance that dissociates into ions when dissolved in water; solution can conduct electrical current
