Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
Biochemistry Test 1
| Question | Answer |
|---|---|
| Units | Fundamental units- describe a fundamental quantity of nature. Derived units- describe a property of nature using two or more fundamental units. |
| Weight | Describes force of gravity between an object & the earth. At earth's surface, mass & weight are interchangeable. Weight of a mass changes in relation to its distance from the earth. Many uses mass & weight interchangeably. |
| Significant digits | Last digit in any measurement is doubtful. A calculated value cannot have more significant digits than the least significant value used in the calculations. Values are rounded off after all calculations. |
| Elements | Matter composed of only one kind of atom. All atoms of the same element have the same atomic number. There are 92 naturally occurring elements. Element symbols- Group A & Transistional's. |
| Atomic Theory | All matter is composed of atoms in constant motion. All atoms of the same element have the same chemical properties. Atoms combine to form molecules. Subatomic particles- atoms are composed of protons, neutrons, & electrons |
| Protons | Located in the nucleus. have a positive charge. number of protons is the atomic number. atomic number determines the number and location of electrons, which determines the chemical properties of an atom. |
| Electrons | Located in energy levels around the nucleus, Bohr model, rejected in 1920's. Have negative charge. Number of electrons = number of protons in a ground state atom. Number and arrangement of electrons determines the chemical properties of atoms. |
| Carbon | Atomic number = 6 and atomic mass number = 12. P level can hold up to six electrons. S levels can only hold up to two electrons. |
| Sodium | Atomic number = 11 and atomic mass number = 23 |
| Periodic table group 2A name the element and its charge Mg, Ca, Ba | Magnesium +2, calcium +2, and barium +2 |
| Periodic table Group 4A name the element and its common charge C. | carbon -4, +4, +2 |
| Periodic table Group 5A name the element and its common charge N and P | Nitrogen -3, Phosphorus -3 |
| Periodic table Group 7A name the element and its common charge F, Cl, Br, I | Fluorine -1, Chlorine -1, Bromine -1, Iodine -1. |
| Name the transition metal and its charge Mo | molybdenum, +2, +3, +4, +5, and +6 |
| Name the transition metal and its charge Mn | manganese, +2, +3, +4, +6, and +7 |
| Name the transition metal and its charge Au | gold, +1, +3 |
| Name the transition metal and its charge Fe | iron, +2, and +3 |
| Name the transition metal and its charge Sn | tin, +2 and +4 |
| wave or quantum mechanics | determines most likely location of electrons. |
| Compound | a combination of elements. can be broken down into constituent elements. elements always in definite proportion by mass and volume. |
| molecule | stable combination of atoms with no charge. |
| ionic bonding | transfer of electrons between metal and nonmetal, readily disassociate in polar solvents & form ions, electrolytes- acids, bases, & salts |
| polyatomic ions | stable combination of atoms that carry charge |
| redox number | valence number or charge number, indicate ability of atoms or polyatomic ions to combine with each other. |
| Avogadro's hypothesis | since elements combine in whole number ratios by volume & since actual mass must be directly proportional to atomic mass, then equal volumes of elements must have equal & constant number of atoms. |
| mole | amount of substance. actual mass divided by atomic mass = mole. a mole of any substance at standard temperature and pressure has the same number of particles as a mole of any other substance. |
| exergonic or exothermic | net release of energy, explosion, eukaryotic respiration |
| Describing | Qualitative- description without measurement, subjective, Quantitative- description with measurement, objective, Measurement- number & unit |
| Accuracy | Closeness of a measurement to the actual quantity being measured. |
| Precision | Consistency of a set of measurements. |
| Neutrons | Located in nucleus. Have a neutral charge. The number of protons plus the number of neutrons equals the atomic mass number of an atom. Atomic mass determines molar mass. |
| Hydrogen | Atomic number 1 and atomic mass 1. The K level can hold 2 electrons. Hydrogen is the least dense and the lightest of all the elements. |
| Oxygen | atomic number = 8 and atomic mass number = 16 |
| Isotopes | Atoms of the same element that have different neutrons. Unstable isotopes emit 3 kinds of radiation: alpha, gamma, and beta. radiation is a result of isotopes. Half-life: time for half of an isotope to transition into a stable atom |
| Periodic law | If elements are sorted by rising atomic number, elements w/ similar properties occur at regular intervals. Atomic numbers determine e- arrangement which determines chemical properties. Chemical properties are a periodic function of atomic number. |
| Periodic table group 1A name the element and its charge H, Na, K. | Hydrogen +1, sodium +1, potassium +1 |
| Periodic table Group 3A name the element and its common charge Al, B. | aluminum +3, boron +3 |
| Periodic table Group 8A name the element and its common charge He, Ne, Ar | Helium 0, Neon 0, Argon 0 |
| Name the transition metal and its charge Se | selenium, +1, +2, +4, and +6 |
| Name the transition metal and its charge Ag | silver, +1 |
| Name the transition metal and its charge Hg | mercury, +1, +2, and 2+2 |
| Electron arrangement | electrons are located in energy levels outside the nucleus of an atom, atomic spectra and orbitals. |
| Pure covalent or covalent bonding | equal sharing of e- between nonmetals, no to slight occasional dipole moment. diatomic elements: H2, O2, N2, F2, Cl2, Br2, & I2. |
| Nonpolar covalent bonding | slightly less than equal of sharing electrons between non-metals. slight or cancelling dipole moments. |
| polar covalent | very much less than equal sharing of electrons between nonmetals, large dipole moments. |
| name the polyatomic ions and their charges. NO3-, CO3-2, MnO4-, | nitrate -1, carbonate -2, sodium permanganate -1 |
| name the polyatomic ions and their charges. NH4+, SO4-2, and PO4-3, | ammonium +1, sulfate -2, phosphate -3 |
| name the polyatomic ions and their charges. C2H3O2-1, OH-1, CN-1 | acetate -1, hydroxide -1, and cyanide -1 |
| oxidation reduction | oxidation- always loss of electrons, in eukaryotic cells done by gain of oxygen &/or loss of hydrogen, reduction- always gain of electrons, in eukaryotic cells done by loss of oxygen &/or gain of introduction. |
| formula mass | multiply atomic mass by the subscript of each element |
| Chemical properties | how atoms combine to form molecules. |
| Periodic table Group 6A name the element and its common charge O and S | Oxygen -2, Sulfur -2. |
| Name the transition metal and its charge Cu | copper, +1, and +2 |
| Name the transition metal and its charge Zn | zinc, +1, +2, and 2+2 |
| Name the transition metal and its charge Pb | lead, +2 and +4 |
| uncertainty principle | electron location can only be described in terms of probability. |
| molecular formula | element symbols show the elements in a compound. subscripts show proportions. positive element or polyatomic ion written first. |
| endergonic or endothermic | require constant input of energy, charging a battery for example, or photosynthesis |
| Fundamental Units | a. Distance- meter, 1m = 100cm = 1000mm b. Mass- kilogram, 1kg = 1000g c. Time- second, 60sec = 1min, 3600sec = 1hr d. Temperature- oC, Celsius; K, Kelvin e. Charge- coulomb, 1coul = 6.25 x 1018 e- or p+ |
| Derived Units | a. Volume- dm3 = liter, cm3 = ml b. Density- mass/volume = grams/milliliter |
| Amount of substance, mole | 1.) For element: grams of element divided by atomic mass of element. 2.) For compound: grams of compound divided by formula mass of compound. |
Created by:
steph2003
Popular Biochemistry sets