Chapter 2.2 Flashcards
Matter
anything that has weight and takes up space. This includes all solids, liquids, and gases in our surroundings as well as in our bodies
Atom
smallest particle of an element that has properties of that element
Elements
The simpliest examples of matter with specific chemical properties
COmpounds
Some elements exist in a pure form, but these and other elements are more commonly parts of chemical combinations
Bulk elements
elements the body requires in large amount - carbon, hydrogen, oxygen, nitrogen, sulfur
Trace Elements
Elements required in small amounts
Ultratrace elements
some elements that are toxic in large amounts, but may be vital in very small amounts
Chemical Bonds
Some atoms can combine with atoms like themselves or with other atoms by forming attractions
Nucleus
A central portion of an atom
Electrons
One or more that constantly move around the nucleus
Protons/Neutrons
Are equal in weight but have different electrical properties.
Atomic Number
The number of protons in the atoms of an element
Atomic Weight
The number of protons plus the number of neurtons in each of an elements atoms
Isotopes
Atoms that have same atomic number but different atomic weights.
Three common forms of atomic radiation
Alpha, Beta, and Gamma
Beta radiation consists..
of much smaller particles that travel faster and more deeply penetrate
Alpha radiation consists
of particles from atomic nuclei , each of which includes two protons and neutrons
Gamma Rradiation consists of
a form of energy similar to x-radiation and is most penetrating form of atomic radiation
Molecules
Two or more atoms may combine to form a distinctive type of particle
Molecular Formula
Shorthand used to depict the numebr and types of atoms in a molecule.
Bonds
Atoms combining with other aroms by forming links. Chemical bonds result from interaction of electrons.
Octet Rule
Atoms react in a way that leaves the outermost shell completely filled with electrons, achieving a more stable structure
Inert
When the outermost electron shells are filled, already have stable structures and are chemicall inactive
Ions
Atoms that gain or lose electrons become electrically charged
Cations
Postively charged ions
Anions
negatively charged ions
Ionic Bonds
Ions with opposite charges attract
Covalent Bond
A chemical bond between aotoms that share electrons
Polar Bond
Unlike an ion, a polar molecule has an equal number of protons and electrons but more of the electrons are at one end of the molecule making that end slightly negative while the other end of the molecule is slightly positive.
Hydrogen Bond
The attraction of the positive hydrogen end of a polar molecular to the negative nitrogen or oxygen end of another polar molecule
Synthesis
When two or more atoms, ions, or molecules bond to form a more complex sturcture as when hydrogen and oxygen atoms bond to form molecules of water, the reaction is called synthesis
Decomposition
If the bonds of a reactant molecule break to form simpler molecules, atoms or ions if the reaction
Exchange Reaction
Parts of two different types of molecules trade positions as bonds are broken and new bondsa re formed
Reversible Reaction
This means the product or products can be changed back to the reactant or reactants
Catalysts
Are molecules that influence the rates of chemical reactions but are not consumed in the process
Dissociate
When ionically bound substances are placed inw ater, the ions are attracted to the positive and negative ends of the water molecules and tend to leave each other or dissociate
Acids
Electrolyte that dissociate to release hydrogen ions inw ater
Bases
Substances that release ions that combine with hydrogen ions
Salts
Bases can react with acids to neutralize them, forming water and electrolytes
Acidic
Solutions with more hydrogen ions
Basic (Alkaline)
solutions with fewer hydrogen ions than hydroxide ions, pH values greater than 7
Alkalemia?
Blood pH of 7.5 to 7.8
Alkalosis?
Makes one feel agitated and dizzy.
Acidemia
Occurs when the blood pH falls to 7.0 to 7.3.
Acidosis
Makes one feel disoriented and fatigued, and breathing may become difficult.
Buffers
chemicals that resist pH change
Organic Compounds
have carbon and hydrogen
inorganic compounds
anything thats not organic
Electrolytes
Inorganic susbtances usually dissolve in water and dissociate forming ions
Nonelectrolytes
Most organic compounds that dissolve in water do not release ions
Solvent
A substance in which other susbtances dissolve. WAter is an important solvent
Solute
A substance dissolved ina solvent, such as water
Solution
The combination of a colvent and any solutes dissolved
Organelles use oxygen to
release energy from nutrient molecules
CO2
is a cimple carbon-containing inorganic compound. It is a waste product of the release of energy during certain metabolic reactions
Organic Substances
Important groups of chemical chemicals in cells including carbohydrates, lipids, proteins, and nucleic acids
Carbohydrates
Provide much of the energy that cells require. They also supply materials to build certain cell structures and they often are stored as reserve energy supplies. Water-soluble. Often have twice as many hydrogen as oxygen.
Simple carbohydrates are
sugars
include monosaccharides and disaccharides
Monosaccharides may include
three to seven carbons in a straight chain or ring.
Disaccharides consist of
two simple sugar building blocks
Polyssaccharides
Complex carbohydrates. Built of simple carbohydrates linked to form larger molecules of different sizes. An example is cellulose.
Electrolyes
A solution that has electrically charged particles (ions), so it conducts an electric current. Substances that release ions in water are this
pH scale measures?
Hydrogen ion concentration
