Biology 1408 Chapter 2

Front 1

Proton

Back 1

Carries a postive charge, or a defined amount of electricity. (P+). Relates to Atomic #.

Front 2

Neutrons

Back 2

Has no charge and is part of the nucleus.

Front 3

Electrons

Back 3

Has a negative charge
(E-). Are always across from one another and attracted to protons but arre repelled by neutrons.

Front 4

Atomic Number

Back 4

Number of protons in the nucleus of its atoms.

Front 5

Mass Number

Back 5

Equal to the number of protons and neutrons.

Front 6

Dmitry Mendeleev

Back 6

1869, arranged the known elements into a repeating pattern based on their chemicla properties(Periodic Table).

Front 7

Inert Elements

Back 7

Vertical column farthest to the right. They have none of their electrons is available for chemical interaction. (Solitary atoms)

Front 8

Isotope's Mass Number

Back 8

A superscript number to the left of an element's symbol.

Front 9

Radioactive Decay

Back 9

A radioactive atom spontaneously emits energy as subatomic particles and x-rays when its nucleus disintegrates; transforms one element into another.

Front 10

Isotopes

Back 10

Atoms with the same number of protons but a different number of neutrons.

Front 11

Energy from radioactive decay:

Back 11

It helps us track the molecule of interest with instruments that detect radioactivity.

Front 12

Radioistotopes

Back 12

Are used in medicine; Uses PET (Positron-Emission Tomography) to form images of body tissues.

Front 13

Chemical Bonding

Back 13

Atoms that have vacancies in the outermost "shell" tend to give up, acquire, or share electrons with other atoms.

Front 14

TRUE/FALSE
Atoms with zero vacancies rarely bond with other atoms.

Back 14

True

Front 15

Molecule

Back 15

Is simply two or more atoms of thesame or different elementsjoined in a chemincal bond.

Front 16

Compounds

Back 16

Are molecules that consist of two or more different elements in proportions that never do vary.

Front 17

Mixture

Back 17

Two or more molecules intermingle without chemically bonding.

Front 18

Ion

Back 18

Atom that has either a positive or negative charge

Front 19

Ionic Bond

Back 19

When two resulting ions may stay close together because they have opposite charges that attract each other. One atom donates and extra electron that the other accepts.

Front 20

Covalent Bond

Back 20

Atoms that share a pair of electrons. They are stable and much stronger than ionic bonds.

Front 21

TRUE/FALSE
A single line that connects two atoms in a structural formula represents two shared electrons in one colvalent bond

Back 21

TRUE

Front 22

Nonpolar Covalent Bond

Back 22

Two identical atoms share electrons equally, and the moleculre shows no difference in charge.

Front 23

Polar Covalent Bond

Back 23

Bond that forms betwwen atoms of different elements. One of the atoms pulls the shared electrons a little toward one end of the bond; slight negative charge.

Front 24

Hydrogen Bond

Back 24

When the negatively charged atom is bound to a different molecule or to a different part of the same molecule, the interaction between it and the hydrogen atom; weak; play crucial roles in structure and function of biological molecules; breaks easily

Front 25

Hydrophilic (Water loving)

Back 25

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