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Gen. Cellular Biology > Ch. 2 > Flashcards

Ch. 2 Flashcards

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1
Q

Element

A

A substance that cannot be broken down to other substances. Matter is made up of elements.

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2
Q

Compound

A

A substance consisting of 2 or more different elements. Combined in a fixed ratio. It has different characteristics than those of its elements.

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3
Q

Essential elements

A

A chemical element required for an organism to survive, grow, & reproduce. Of the 92% natural elements, 20-25% are essential elements.

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4
Q

What are the elements that make up 96% of living matter?

A

The element Oxygen, Carbon, Hydrogen, & Nitrogen. The remaining 4% is Calcium, Phosphorus, Potassium, & Sulfur.

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5
Q

Atom

A

The smallest unit of matter that still retains the properties of an element.

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6
Q

Subatomic particles

A

Neutrons, protons, & electrons. They compose the atom.

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7
Q

Where are the subatomic particles located?

A

Protons & neutrons in the nucleus. Electrons form electron clouds around the nucleus.

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8
Q

Daltons

A

A measure of mass for atoms & subatomic particles; the same as the atomic mass unit of amu.

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9
Q

Atomic number

A

The number of protons in nucleus of atom. It is written in as a subscript to the left of the element symbol.

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10
Q

Mass number

A

The sum of protons & neutrons in the nucleus of an atom. Written to the left of element symbols as superscript.

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11
Q

Atomic mass

A

The total mass of an atom.

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12
Q

Isotopes

A

A variation of an element that has different number of neutrons, but still the same number of protons.

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13
Q

Radioactive isotope

A

An isotope in which the nucleus decays spontaneously, giving of particles & energy.

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14
Q

How to find number of neutrons in element?

A

Atomic mass - number of protons.

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15
Q

Half-life

A

The amount of time it takes for 50% of a sample of a radioactive isotope to decay.

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16
Q

Radiometric dating

A

A method for determining the absolute age of rocks & fossils based on the half life of radioactive isotopes.

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17
Q

Energy

A

A capacity to cause change.

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18
Q

Potential energy

A

The energy that matter possesses because of its location or structure.

19
Q

Electron shells

A

Energy levels where electrons are located.

20
Q

Valence electrons

A

Electrons in the outer most shell (valence shell). Determines reactivity. Full valence shell=chemically inert. Inert=chemically unreactive.

21
Q

Orbital

A

3rd space where electrons are found 90% of the time.

22
Q

Chemical bond

A

A mutual attraction between 2 atoms resulting from redistribution of outer electrons.

23
Q

Covalent bond

A

When elements bond by sharing electrons, a pair of valence electrons, by 2 atoms.

24
Q

Structural formula

A

Notation used to represent atoms & bonding. Ex. H-H, O=O.

25
Q

Molecular formula

A

Gives number of atoms of each element present. Ex. H2O.

26
Q

Valence

A

The bonding capacity of a given atom, usually equals the number of unpaired electrons required to complete the valence shell.

27
Q

Electronegativity

A

Measure of the tendency of an atom to attract a bonding pair of electrons. The more electronegative the atom is, the stronger it pulls shared electrons toward itself.

28
Q

Nonpolar covalent bond

A

A type of covalent bond in which electrons are shared equally between 2 atoms of similar electronegativity.

29
Q

Water is what kind of molecule?

A

Water is a polar molecule.

30
Q

Polar covalent bond

A

A covalent bond between atoms that differ in electronegativity. The shared electrons are pulled closer to the electronegative atom.

31
Q

Ion

A

An atom or group of atoms that has gained or lost one or more electrons, thus acquiring change.

32
Q

Cation

A

A positively charged ion. To become a cation the atom has to lose electrons, therefore giving it an overall positive charge. Ex. K+, it loses an electron because it want to have the closest thing to a noble gas. The noble gas closest to it is Ar. So it has to lose an electron to have the same number of valence electrons.

33
Q

Anion

A

A negatively charge ion. The atoms gains electrons so it gives the atom an overall negative charge. Ex. Cl-, it gains an electron because it wants to be like Ar.

34
Q

Ionic bond

A

A chemical bond resulting from the attraction between oppositely charged ions.

35
Q

Ionic compounds

A

Compounds formed by ionic bonds.

36
Q

Hydrogen bond

A

A type of weak chemical bond that is formed when slightly positive hydrogen atom of a polar covalent bond in one molecule is attracted to a slightly negative atom of a polar covalent bond.

37
Q

Van der Waals interactions

A

Weak attractions between molecule or parts of molecules that result from transient local partial charges. Attractions between molecule that are close together.

38
Q

Reactants(reagents)

A

The things that react. The starting molecules of a chemical reaction.

39
Q

Product

A

What is produced from the reactants. The final molecules of a chemical reaction.

40
Q

What is conserved in a chemical reaction?

A

Matter is concerned in a chemical reaction. Relations cannot create or destroy atoms, but can only rearrange the electrons among them.
All chemical reactions are reversible.

41
Q

Chemical equilibrium

A

The point which reactions off set one another exactly. When the forward and reverse reaction rates are equal.

42
Q

Chemical reaction

A

The making and breaking of chemical bonds.

43
Q

Matter

A

Anything that takes up space & has mass. Organisms are composed of matter.

Gen. Cellular Biology (6 decks)

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