Human Anatomy & Physiology (chapter 2) isbn:0070272468
Terms
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- Each one carries a single positive charge
- protons
- bio-
- life
- di-
- two
- glyc-
- sweet
- iso-
- equal
- lip-
- fat
- -lyt
- dissolvable
- mono-
- one
- sacchar-
- sugar
- syn-
- together
- -valent
- having power
- Body functions depend on -----------
- cellular functions
- Cellular functions result from__________ changes
- chemical
- A life science called biological chemistry
- biochemistry
- Anything that has weight and takes up space
- matter
- All matter is composed of fundamental substances called
- elements
- chemical combinations of elements
- compounds
- elements required by the body in large amounts are called
- bulk elements
- Some elements that are toxic in large amounts but vital in very small amounts.
- Ultratrace elements
- The smallest complete units of elements
- Atoms
- Components of an atom:__&________
- Nucleus and electrons
- Small, with almost no weight and carry a charge that is ________
- negative
- Symbol Cl
- Chlorine
- Uncharged (electrically neutral) particle found in the nucleus
- neutron
- A particle that is electrically charged because it gained or lost one or more electrons.
- ion
- Formed by the chemical union of two or more atoms.
- molecule
- symbol O
- oxygen
- symbol C
- carbon
- symbol H
- hydrogen
- symbol N
- nitrogen
- symbol P
- phosphorus
- symbol K
- Potassium
- symbol S
- Sulfur
- Symbol Na
- Sodium
- symbol Mg
- magnesium
- symbol Co
- cobalt
- symbol Cu
- copper
- Symbol F
- Fluorine
- symbol I
- iodine
- symbol Fe
- Iron
- symbol Mn
- Manganese
- symbol Zn
- zinc
- Activity that forms or breaks bonds of atoms, ions or molecules___________ ___________
- chemical reaction
- Those being changed by chemical reactions
- Reactants
- Those formed by reactions' conclusions
- Products
- When bonds break to form simpler ions, atoms or molecules
- decomposition
- symbol of synthesis
- A + B (ra) AB
- variance in the atomic weight of an element is caused by the variance of the number of____
- neutrons
- What largely influences the interactions of atoms?
- Number of electrons
- T/F All isotopes of an atom chemically react in the same manner.
- True because they have the same number of electrons. Electrons determine the interactions.
- Unstable isotopes that will release energy or pieces of themselves are said to be_________
- radioactive
- Energy or atomic fragments released by unstable isotopes is called_____
- atomic radiation
- Three common forms of atomic radiation include
- alpha beta & gamma
- This radiation consists of very small particles (electrons), moves fast and can deeply penetrate matter.
- beta
- The most penetrating common form of radiation
- Gamma
- Gamma radiation is similar to
- X-radiation
- What is used to depict the numbers and kind of atoms in a molecule?
- Molecular formula
- When atoms of the same element combine, what are they called?
- a Molecule of that element
- If atoms of different elements combine, what are they called?
- compounds
- When atoms combine by forming bonds, they do what 3 possible things with electrons?
- gain, lose or share electrons
- The regions of space around a nucleus are called___________
- shells
- For atomic number 18 (or under) what is max electrons in 1st three shells?
- 18
- chemically inactive
- inert
- outermost electron shells are filled in these atoms
- inert
- atoms with incompletely filled outer shells tend to _________ _________ or _________ electrons
- gain lose or share electrons
- atoms that gain or lose electrons
- ions
- symbol Na+
- sodium ion with a positive charge of +1
- symbol cl-
- chloride ion with a negative charge -1
- Oppositely charged ions ______________
- attract
- electrovalent bond
- ionic bond
- Example of ionic bond
-
Sodium positive and chlorine negative
Na+ and Cl- unite to become NaCl (table salt) - Term when atoms bond by sharing electrons
- Covalent bonding
- When one pair of electrons are shared in bonding
- Single covalent bond
- When two pair of electrons are shared in bonding
- double covalent bond
- The anomaly existing in a polar molecule
- One atom slightly negative and another slightly positive.
- Where do the polar covalent bonds typically occur?
- Where hydrogen bonds to oxygen or nitrogen
- Why are polar molecules soluble in water?
- Because water molecules themselves are polar.
- The attraction of positive hydrogen of one polar molecule to the negative nitrogen or oxygen of another polar molecule is called ________ _______________
- hydrogen bond
- Usually atoms of each element form specific numbers of _________ ________
- chemical bonds
- hydrogen atoms form how many chemical bonds?
- only one
- oxygen atoms form how many chemical bonds?
- two
- Nitrogen atoms form how many chemical bonds?
- three
- Carbon atoms form how many chemical bonds?
- four
- Single lines or double lines used to represent respective bonds, are called ____________ ____________
- structural formulas
- Radiation that adds or removes electrons from atoms is called
- ionizing radiation
- SYMBOL OF DECOMPOSITION
- AB (ra) A + B
- Reactions particularly important in growth and repair
- Synthesis
- Reactions when food stuffs are digested and release energy
- Decomposition
- synonym for exchange reaction
- replacement reaction
- Symbol for exchange reaction
- AB + CD (ra) AD + CB
- Reaction when parts of two kinds of molecules trade positions
- Exchange reaction
- Example of exchange reaction
- Acid reacting with a base to produce water and salt
- Molecules that influence rates of reactions but are not consumed in the process
- Catalysts
- What does the polarity of water cause in ionically bound salts?
- The salts dissociate from one another NaCl becomes Na+ + Cl-
- Substances that release ions in water
- electrolytes
- Electrolytes that release hydrogen ions in water
- Acids
- symbol of reaction wherein electrolytes create acid by releasing hydrogen ions in water
- HCl becomes H+ + Cl-
- Electrolyte ions that combine with hydrogen ions in water
- bases
- Example of electrolyte that releases ions that combine with hydrogen to form a base
- NaOH (yields) Na+ + OH-
- Acids and bases can react to form water and electrolytes (called _____)
- salts
- Example of reaction of acid and base to create water and salt
- HCl + NaOH (ra) H2O + NaCl
- Three types of electrolytes ___ __ ___
- acids, bases, salts
- In acids (hydrogen ions ) what unit of measure tells us its concentration?
- grams of ions per liter of solution
- Shorthand system for acid concentration (grams of ions per liter of solution)
- pH scale
- As hydrogen ion concentration increases the pH number______________
- Decreases (becomes more acidic)
- What is the size increase or decrease between each whole number on the pH scale?
- Tenfold
- Because water ionizes to release equal acid and base ions, it is said to be _____________
- neutral
- What is the pH of neutral water
- pH is 7.0
- What is the complete range of the pH scale
- 0 to 14
- egg white pH
- 8.0
- hominy pH
- 7.7
- human blood pH
- 7.4
- sodium bicarbonate pH
- 8.4
- borax pH
- 9.2
- milk of magnesia pH
- 10.5
- household ammonia pH
- 11.5
- cows milk pH
- 6.6
- dates pH
- 6.2
- corn pH
- 6.0
- white bread pH
- 5.5
- cabbage pH
- 5.3
- carrots pH
- 5.0
- banana pH
- 4.6
- tomato juice pH
- 4.2
- grapes pH
- 4.0
- sauerkraut pH
- 3.5
- apple juice pH
- 3.0
- vinegar pH
- 2.4
- lemon juice pH
- 2.3
- gastric juice pH
- 2.0
- Example of water ionizing to become neutral
- H2O (ra) H+ + OH-
- When pH changes out of its natural range in the body the result is ___________
- illness
- Severe vomiting that would empty the alkaline small intestines would cause _______________
- acidosis
- Mild vomiting that depletes stomach acid would cause_____________
- alkalosis
- Two large groups of chemicals regarding metabolism__________ and_________
- organic and inorganic
- Most metabolic reactions occur in
- water
- Blood is mostly___________
- water
- The substance in blood that enables it to absorb and carry heat
- water
- Name four inorganic substances found in cells (w, o, cd, i.s.)
- water, oxygen, carbon dioxide and inorganic salts
- A complete atom has no charge because the number of electrons and protons are__________
- equal
- A solution that contains electrically charged particles (ions) will conduct an ____________ ____________
- electric current
- Because they dissolve in water or react in water to produce ions, inorganic chemicals are
- electrolytes
- Electrically uncharged particle of the nucleus
- Neutron
- Elements required in small amounts by the body are called__
- trace elements
- How many of the elements can be called naturally occurring matter?
- 92
- Inert atoms cannot form ____________ __________
- chemical bonds
- Large particle found within the nucleus,carries a positive charge and is relatively large.
- proton
- Name of the reaction when two or more ions, atoms, or molecules bond into a more complex structure
- synthesis
- Organic chemicals that dissolve in water do not release ions and are called
- nonelectrolytes
- Otherwise very different, protons and neutrons are about equal in ___
- weight
- Smallest particle of an element that has the properties of that element
- atom
- The number of protons in an atom, delineates its _________ ___________
- Atomic number
- The radiation that emits two neutrons and two protons, moves slowly and does not penetrate matter easily is called
- Alpha radiation
- The six bulk elements include carbon oxygen and hydrogen and also N_________,S________ and P_________.
- nitrogen, sulfur and phosphorus
- The sum of the number of protons and neutrons in an atom essentially equal its __________ ___________
- atomic weight
- What does the subscript of an atom indicate?
- The number of atoms of a specific type in a given formula.
- What is the maximum electron total in the 1st three shells of an element having 18 or less electrons
- 18 2 in 1st and 8 in each subsequent shell.
- When atoms have the same atomic number but different atomic weight they are called _____
- isotopes
- Why is the nucleus always positively charged?
- It contains protons
- extremely small particle with a negative electrical charge, almost no weight and in constant motion around a nucleus.
- electron
- nucle-
- kernel
- A molecule that has equal numbers of electrons and protons but one atom has more than its share of electrons
- polar molecule
- Large particles of the nucleus
- Protons and usually Neutrons
- Examples of bases s h,p h,m h,s b
-
sodium hydroxide
potassium hydroxide
magnesium hydroxide
sodium bicarbonate - Blood pH of 7.5 to 7.8
- alkalosis
- formula carbon dioxide
- CO2
- formula chloride ions
- Cl-
- formula potasium ions
- K+
- Functions of water
-
Major component of body fluids
Medium in which most biochemical
reactions occur.
Transports various chemical substances
Helps regulate body temperature - Function of bicarbonate ions (HCO3-
- help maintain acid base balance
- acid examples c,h,a,p
-
carbonic acid
hydrochloric acid
acetic acid
phosphoric acid - Examples of salt s c, a c, m s.
-
sodium chloride
aluminum chloride
magesium sulfate - Blood pH of 7.0 to 7.3
- Acidosis
- Formula Bicarbonate ions
- HCO3-
- formula Hydrogen ions
- H+
- Formula Sodium ions
- Na+
- Function of Oxygen
- Used in release of energy in glucose molecules
- Function of carbonate ions (CO3-2)
- component of bone tissue
- Chloride ions (Cl-)
- Help maintain water balance
- Function of hydrogen ions (H+)
- pH of the internal environment
- Sulfate ions (SO4-2)
-
Help maintain polarization of cell membranes
acid-base balance - Carbohydrates classified by ____.
-
Size: either simple or
complex - Acid characteristic
- Substance that releases hydrogen ions
- solutions with more hydrogen ions than hydroxyl ions are _____________
- acidic
- symbol water
- H2O
- formula calcium ions
- Ca+2
- Formula magnesium ions
- Mg+2
- formula sulfate ions
- SO4-2
- Magnesium ions (Mg+2)
-
Component of bone tissue
required for certain metabolic processes. - Funtion of Phosphate ions (PO4-3)
-
Required for synthesis of ATP
nucleic acids
vital substances
component of bone tissue
Help maintain polarization of cell membranes. - Function of Potassium ions (K+)
- Required for polarization of cell membranes
-
Important groups of organic substances in cells include c_________
l_________
p_________
n_________ a______ -
carbohydrates
lipids
proteins
nucleic acids - characteristic of base
- Substance that releases ions that can combine with hydrogen ions
- characteristic of salt
- substance formed by the reaction between an acid and a base
- Solution with fewer hydrogen ions than hydroxyl ions
- basic
- formula oxygen
- O2
- formula carbonate ions
- CO3-2
- formula Phosphate ions
- PO4-3
- Function of carbon dioxide (CO2)
- Waste product that results from metabolism
- Function of Calcium ions (Ca+2
-
Necessary for bone developement
Muscle contraction
Blood clotting - Function of sodium ions (Na+)
-
Required for polarization of cell membranes
Help maintain water balance - In carbohydrates the usual ratio of hydrogen to oxygen (give examples)
-
2 to 1
IE:Glucose C6 H12 O6
sucrose C12 H22 O11 - A polysaccharide similar to starch that is synthesized by animals (including humans)
- glycogen
- Another name for complex carbohydrates built from many simple carbohydrates.
- polysaccharides
- a common name for simple carbohydrates
- sugars
- A single sugar: carbohydrate.
- Monosaccharide
- A double sugar: simple carbohydrate
- disaccharide
- Its molecules consist of branched chains of sugar units.
- glycogen
- Glucose (dextrose), fructose and galactose are__
- monosaccharides
- Monosaccharides include 3 to 7 carbon atoms and are structured in a ________ ______ or a ____.
- Straight chain or a ring
- Disaccharides consist of 2 ___ _______ units.
- six carbon units
- Examples of disaccharides include _______ and ________
-
sucrose (table sugar)
and
lactose (milk sugar) -
Picture
C6 H12 O6 - monosaccharide (glucose) may have a straight chain of carbon atoms
- glucose is also called
- dextrose
-
picture
This shape symbolizes what - ring structure of a glucose molecule
- What is the solubility characteristic of lipids?
- organic chemical soluble in organic liquids but insoluble in water.
- Most common lipids
- fats
- Primary use of fats
- supply energy for cellular activities
- Contrast Fats Hydrogen Oxygen ratio with that of carbohydrates. Example:
- Fats have a much lower oxygen ration than carbs. (The fat Tristearin: C57 H110 O6)
-
The building blocks of fat molecules
______ _______and___________ - Fatty acids and glycerol
- Of every fat molecule, one portion is always the same.
- The glycerol portion is the same in all fat molecules.
- At the end of the chain of carbon atoms, all fatty acids include a ________ group: (symbol).
- Carboxyl group (-COOH)
- What is characteristic of a saturated fatty acid?
- The carbon atoms are linked by single carbon-carbon bonds and each carbon atom binds as many hydrogen atoms as posible and thusly are SATURATED with hydrogen atoms.
- What is charasteristic of monounsaturated fatty acids?
- They are not 100% saturated with hydrogen atoms because there is one (mono) bonding that is double bonding between carbon-carbon atoms rather than all single bonded.
- What is characteristic if poly unsaturated fatty acids?
- They have two or more double bonds of carbon and thusly cant get maximally saturated with hydrogen atoms as in a single carbon-carbon bonding situation.
- How are fatty acids and glycerol united?
- Each glycerol molecule combines with three fatty acids. (triglyceride)
- Fat molecules that contain only the saturated fatty acids:
- Saturated fats
- Fat molecules that include unsaturated fatty acids are calle____________
- unsaturated fats