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102 Cards in this Set
- Front
- Back
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A small, very toxic molecule (NH3) produced by nitrogen fixation or as a metabolic waste product of protein and nucleic acid metabolism.
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ammonia
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(an´-i-on) A negatively charged ion.
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anion
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The smallest unit of matter that retains the properties of an element.
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atom
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The total mass of an atom, which is the mass in grams of 1 mole of the atom.
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atomic mass
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An atom’s dense central core, containing protons and neutrons.
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atomic nucleus
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The number of protons in the nucleus of an atom, unique for each element and designated by a subscript to the left of the elemental symbol.
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atomic number
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An attraction between two atoms, resulting from a sharing of outer-shell electrons or the presence of opposite charges on the atoms. The bonded atoms gain complete outer electron shells.
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cation
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An attraction between two atoms, resulting from a sharing of outer-shell electrons or the presence of opposite charges on the atoms. The bonded atoms gain complete outer electron shells.
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chemical bond
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In a chemical reaction, the state in which the rate of the forward reaction equals the rate of the reverse reaction, so that the relative concentrations of the reactants and products do not change with time.
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chemical equilibrium
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The making and breaking of chemical bonds, leading to changes in the composition of matter.
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chemical reaction
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A substance consisting of two or more different elements combined in a fixed ratio.
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compound
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(ko-va´-lent) A type of strong chemical bond in which two atoms share one or more pairs of valence electrons.
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covalent bond
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A measure of mass for atoms and subatomic particles; the same as the atomic mass unit, or amu.
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dalton
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A double covalent bond; the sharing of two pairs of valence electrons by two atoms.
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double bond
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A subatomic particle with a single negative electrical charge and a mass about 1/2,000 that of a neutron or proton. One or more electrons move around the nucleus of an atom.
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electron
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An energy level of electrons at a characteristic average distance from the nucleus of an atom.
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Electron shell
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The attraction of a given atom for the electrons of a covalent bond.
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electronegativity
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Any substance that cannot be broken down to any other substance by chemical reactions.
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Element
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The capacity to cause change, especially to do work (to move matter against an opposing force).
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energy
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A type of weak chemical bond that is formed when the slightly positive hydrogen atom of a polar covalent bond in one molecule is attracted to the slightly negative atom of a polar covalent bond in another molecule.
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hydrogen bond
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(i´-on) An atom or group of atoms that has gained or lost one or more electrons, thus acquiring a charge.
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ion
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(i-on´-ik) A chemical bond resulting from the attraction between oppositely charged ions.
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ionic bond
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A compound resulting from the formation of an ionic bond; also called a salt.
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ionic compound
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A type of molecular notation representing the quantity of constituent atoms, but not the nature of the bonds that join them.
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molecular formula
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Two or more atoms held together by covalent bonds.
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molecule
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A subatomic particle having no electrical charge (electrically neutral), with a mass of about 1.7 × 10-24 g, found in the nucleus of an atom.
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neutron
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A type of covalent bond in which electrons are shared equally between two atoms of similar electronegativity.
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nonpolar covalent bond
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(1) An atom’s central core, containing protons and neutrons. (2) The chromosome-containing organelle of a eukaryotic cell. (3) A cluster of neurons.
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nucleus
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The three-dimensional space where an electron is found 90% of the time.
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orbital
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A covalent bond between atoms that differ in electronegativity. The shared electrons are pulled closer to the more electronegative atom, making it slightly negative and the other atom slightly positive.
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polar covalent bond
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(i´-so-top´) One of several atomic forms of an element, each with the same number of protons but a different number of neutrons, thus differing in atomic mass.
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isotope
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The sum of the number of protons and neutrons in an atom’s nucleus
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mass number
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Anything that takes up space and has mass.
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matter
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The energy that matter possesses as a result of its location or spatial arrangement (structure).
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potential energy
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A material resulting from a chemical reaction.
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product
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(pro´-ton) A subatomic particle with a single positive electrical charge, with a mass of about 1.7 × 10-24 g, found in the nucleus of an atom.
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proton
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An isotope (an atomic form of a chemical element) that is unstable; the nucleus decays spontaneously, giving off detectable particles and energy.
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radioactive isotope
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A starting material in a chemical reaction.
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reactant
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A compound resulting from the formation of an ionic bond; also called an ionic compound.
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salt
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A single covalent bond; the sharing of a pair of valence electrons by two atoms.
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single bond
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(i´-so-top´) One of several atomic forms of an element, each with the same number of protons but a different number of neutrons, thus differing in atomic mass.
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isotope
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The sum of the number of protons and neutrons in an atom’s nucleus
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mass number
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Anything that takes up space and has mass.
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matter
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The energy that matter possesses as a result of its location or spatial arrangement (structure).
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potential energy
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A material resulting from a chemical reaction.
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product
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(pro´-ton) A subatomic particle with a single positive electrical charge, with a mass of about 1.7 × 10-24 g, found in the nucleus of an atom.
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proton
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An isotope (an atomic form of a chemical element) that is unstable; the nucleus decays spontaneously, giving off detectable particles and energy.
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radioactive isotope
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A starting material in a chemical reaction.
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reactant
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A compound resulting from the formation of an ionic bond; also called an ionic compound.
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salt
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A single covalent bond; the sharing of a pair of valence electrons by two atoms.
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single bond
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A type of molecular notation in which the constituent atoms are joined by lines representing covalent bonds.
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structural formula
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An explanation that is broad in scope, generates new hypotheses, and is supported by a large body of evidence.
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Theory
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An element indispensable for life but required in extremely minute amounts.
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Trace element
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The bonding capacity of a given atom; usually equals the number of unpaired electrons required to complete the atom’s outermost (valence) shell.
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valence
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A type of molecular notation in which the constituent atoms are joined by lines representing covalent bonds.
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structural formula
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An electron in the outermost electron shell.
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valence electron
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An explanation that is broad in scope, generates new hypotheses, and is supported by a large body of evidence.
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Theory
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The outermost energy shell of an atom, containing the valence electrons involved in the chemical reactions of that atom.
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valence shell
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A type of molecular notation in which the constituent atoms are joined by lines representing covalent bonds.
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structural formula
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Weak attractions between molecules or parts of molecules that result from localized charge fluctuations.
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van der Waals interactions
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An element indispensable for life but required in extremely minute amounts.
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Trace element
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A type of molecular notation in which the constituent atoms are joined by lines representing covalent bonds.
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structural formula
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The bonding capacity of a given atom; usually equals the number of unpaired electrons required to complete the atom’s outermost (valence) shell.
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valence
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An explanation that is broad in scope, generates new hypotheses, and is supported by a large body of evidence.
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Theory
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An explanation that is broad in scope, generates new hypotheses, and is supported by a large body of evidence.
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Theory
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An element indispensable for life but required in extremely minute amounts.
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Trace element
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An electron in the outermost electron shell.
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valence electron
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An element indispensable for life but required in extremely minute amounts.
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Trace element
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The outermost energy shell of an atom, containing the valence electrons involved in the chemical reactions of that atom.
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valence shell
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The bonding capacity of a given atom; usually equals the number of unpaired electrons required to complete the atom’s outermost (valence) shell.
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valence
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The bonding capacity of a given atom; usually equals the number of unpaired electrons required to complete the atom’s outermost (valence) shell.
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valence
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Weak attractions between molecules or parts of molecules that result from localized charge fluctuations.
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van der Waals interactions
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An electron in the outermost electron shell.
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valence electron
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An electron in the outermost electron shell.
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valence electron
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The outermost energy shell of an atom, containing the valence electrons involved in the chemical reactions of that atom.
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valence shell
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The outermost energy shell of an atom, containing the valence electrons involved in the chemical reactions of that atom.
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valence shell
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Weak attractions between molecules or parts of molecules that result from localized charge fluctuations.
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van der Waals interactions
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Weak attractions between molecules or parts of molecules that result from localized charge fluctuations.
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van der Waals interactions
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In the term trace element, the modifier trace means
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the element is required in very small amounts.
the element can be used as a label to trace atoms through an organism's metabolism. the element is very rare on Earth. the element enhances health but is not essential for the organism's long-term survival. the element passes rapidly through the organism. |
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Compared with 31P, the radioactive isotope 32P has
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a different atomic number.
one more neutron. one more proton. one more electron. a different charge. |
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Atoms can be represented by simply listing the number of protons, neutrons, and electrons—for example, 2p+; 2n0; 2e– for helium. Which one of the following lists represents the 18O isotope of oxygen?
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6p+; 8n0; 6e–
8p+; 10n0; 8e– 9p+; 9n0; 9e– 7p+; 2n0; 9e– 10p+; 8n0; 9e– |
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The atomic number of sulfur is 16. Sulfur combines with hydrogen by covalent bonding to form a compound, hydrogen sulfide. Based on the number of valence electrons in a sulfur atom, predict the molecular formula of the compound:
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HS
HS2 H2S H3S2 H4S |
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The reactivity of an atom arises from
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the average distance of the outermost electron shell from the nucleus.
the existence of unpaired electrons in the valence shell. the sum of the potential energies of all the electron shells. the potential energy of the valence shell. the energy difference between the s and p orbitals. |
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In the term trace element, the modifier trace means
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the element is required in very small amounts.
the element can be used as a label to trace atoms through an organism's metabolism. the element is very rare on Earth. the element enhances health but is not essential for the organism's long-term survival. the element passes rapidly through the organism. |
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Which statement is true of all atoms that are anions?
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The atom has more electrons than protons.
The atom has more protons than electrons. The atom has fewer protons than does a neutral atom of the same element. The atom has more neutrons than protons. The net charge is 1–. |
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Compared with 31P, the radioactive isotope 32P has
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a different atomic number.
one more neutron. one more proton. one more electron. a different charge. |
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What coefficients must be placed in the following blanks so that all atoms are accounted for in the products?
C6H12O6 → _____ C2H6O + _____CO2 |
1; 2
2; 2 1; 3 1; 1 3; 1 |
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Atoms can be represented by simply listing the number of protons, neutrons, and electrons—for example, 2p+; 2n0; 2e– for helium. Which one of the following lists represents the 18O isotope of oxygen?
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6p+; 8n0; 6e–
8p+; 10n0; 8e– 9p+; 9n0; 9e– 7p+; 2n0; 9e– 10p+; 8n0; 9e– |
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Which of the following statements correctly describes any chemical reaction that has reached equilibrium?
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The concentrations of products and reactants are equal.
The rates of the forward and reverse reactions are equal. Both forward and reverse reactions have halted. The reaction is now irreversible. No reactants remain. |
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The atomic number of sulfur is 16. Sulfur combines with hydrogen by covalent bonding to form a compound, hydrogen sulfide. Based on the number of valence electrons in a sulfur atom, predict the molecular formula of the compound:
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HS
HS2 H2S H3S2 H4S |
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In the term trace element, the modifier trace means
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the element is required in very small amounts.
the element can be used as a label to trace atoms through an organism's metabolism. the element is very rare on Earth. the element enhances health but is not essential for the organism's long-term survival. the element passes rapidly through the organism. |
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Compared with 31P, the radioactive isotope 32P has
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a different atomic number.
one more neutron. one more proton. one more electron. a different charge. |
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Atoms can be represented by simply listing the number of protons, neutrons, and electrons—for example, 2p+; 2n0; 2e– for helium. Which one of the following lists represents the 18O isotope of oxygen?
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6p+; 8n0; 6e–
8p+; 10n0; 8e– 9p+; 9n0; 9e– 7p+; 2n0; 9e– 10p+; 8n0; 9e– |
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The reactivity of an atom arises from
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the average distance of the outermost electron shell from the nucleus.
the existence of unpaired electrons in the valence shell. the sum of the potential energies of all the electron shells. the potential energy of the valence shell. the energy difference between the s and p orbitals. |
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Which statement is true of all atoms that are anions?
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The atom has more electrons than protons.
The atom has more protons than electrons. The atom has fewer protons than does a neutral atom of the same element. The atom has more neutrons than protons. The net charge is 1–. |
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The atomic number of sulfur is 16. Sulfur combines with hydrogen by covalent bonding to form a compound, hydrogen sulfide. Based on the number of valence electrons in a sulfur atom, predict the molecular formula of the compound:
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HS
HS2 H2S H3S2 H4S |
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The reactivity of an atom arises from
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the average distance of the outermost electron shell from the nucleus.
the existence of unpaired electrons in the valence shell. the sum of the potential energies of all the electron shells. the potential energy of the valence shell. the energy difference between the s and p orbitals. |
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What coefficients must be placed in the following blanks so that all atoms are accounted for in the products?
C6H12O6 → _____ C2H6O + _____CO2 |
1; 2
2; 2 1; 3 1; 1 3; 1 |
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Which statement is true of all atoms that are anions?
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The atom has more electrons than protons.
The atom has more protons than electrons. The atom has fewer protons than does a neutral atom of the same element. The atom has more neutrons than protons. The net charge is 1–. |
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Which of the following statements correctly describes any chemical reaction that has reached equilibrium?
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The concentrations of products and reactants are equal.
The rates of the forward and reverse reactions are equal. Both forward and reverse reactions have halted. The reaction is now irreversible. No reactants remain. |
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What coefficients must be placed in the following blanks so that all atoms are accounted for in the products?
C6H12O6 → _____ C2H6O + _____CO2 |
1; 2
2; 2 1; 3 1; 1 3; 1 |
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Which of the following statements correctly describes any chemical reaction that has reached equilibrium?
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The concentrations of products and reactants are equal.
The rates of the forward and reverse reactions are equal. Both forward and reverse reactions have halted. The reaction is now irreversible. No reactants remain. |
