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Campbell biology in focus, 3rd edition test exam bank chapter 002 complete solution 2024 verified
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Campbell biology in focus, 3rd edition test exam bank chapter 002 complete solution 2024 verified
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Campbell Biology in Focus - Chapter 21. matter: Anything that takes up space and has mass.
2. element: Any substance that cannot be broken down to any other substance by
chemical reactions.
3. compound: A substance consisting of two or more different elements
combined in a fixed ratio.
4. emergent properties: Properties not possessed by the constituents.
5. What four elements make up 96% of living matter?: carbon, hydrogen,
oxygen, nitrogen
6. essential element: A chemical element required for an organism to survive,
grow, and reproduce.
7. trace element: An element indispensable for life but required in extremely
minute amounts.
8. atom: The smallest unit of matter that retains the properties of an element.
9. subatomic particles: The parts that make up an atom.
10. neutron: A subatomic particle having no electrical charge (electrically
neutral), with a mass of 1 dalton, found in the nucleus of an atom.
11. proton: A subatomic particle with a single positive electrical charge, with a
mass of 1 dalton, found in the nucleus of an atom.
12. electron: A subatomic particle with a single negative charge and a minute
mass, and move around the nucleus of an atom.
13. atomic nucleus: An atom's dense central core, containing protons and
neutrons.
14. dalton: A measure of mass for atoms and subatomic particles; the same as
the atomic mass unit, or amu.
15. atomic number: The number of protons in the nucleus of an atom, unique
for each element and designated by a subscript.
16. mass number: The sum of the number of protons and neutrons in an atom's
nucleus.
17. atomic mass: The total mass of an atom, which is the mass in grams of 1
mole of the atom.
18. isotope: 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.
19. radioactive isotope: An isotope that is unstable; the nucleus decays
spontaneously, giving off detectable particles of energy.
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, 20. energy: The capacity to cause change, especially to do work (to move
matter against an opposing force).
21. potential energy: The energy that matter possesses as a result of its
location or spatial arrangement (structure).
22 electron shell: An energy level of electrons at a characteristic average
distance from the nucleus of an atom.
23. periodic table of the elements: A tabular arrangement of the chemical
elements, organized on the basis of their atomic number (number of protons in
the nucleus), electron configurations, and recurring chemical properties.
24. period: A row of the periodic table, corresponding to all of the atoms with that
number of electron shells.
25. group: A column of the periodic table, each having the sequential addition of
an electron and a proton moving from left-to-right.
26. valence electron: An electron in the outermost electron shell.
27. valence shell: The outermost energy shell of an atom, containing the valence
electrons involved in the chemical reactions of that atom.
28. inert: Chemically unreactive because the valence shell is full.
29. chemical bond: An attraction between two atoms, resulting from a sharing of
outer shell electrons or the presence of opposite charges on the atoms.
30. covalent bond: A type of strong chemical bond in which two atoms share one
or more pairs of valence electrons.
31. molecule: Two or more atoms held together by covalent bonds.
32. molecular formula: A way to represent just the atoms of a molecule.
33. structural formula: A way to represent the atoms of a molecule, and the
bonds with lines.
34. single bond: The sharing of a pair of valence electrons by two atoms.
35. double bond: The sharing of two pairs of valence electrons by two atoms.
36. valence: The bonding capacity of a given atom; the number of covalent bonds
an atom can form usually equals the number of unpaired electrons in its
outermost shell.
37. electronegativity: The attraction of a given atom for the electrons of a
covalent bond.
38. nonpolar covalent bond: A type of bond in which electrons are shared
equally between two atoms of similar electronegativity.
39. polar covalent bond: A 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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