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General Biology I E1 > Chapter 2 > Flashcards

Chapter 2 Flashcards

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1
Q

Matter

A
  • anything that takes up space and has mass
  • made up of elements
  • consists of chemical elements in pure form and in combinations called compounds
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2
Q

Elements

A

substances that cannot be broken down to other substances by chemical reactions

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3
Q

Structure

A

helps dictate the function

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4
Q

Compound

A
  • a substance consisting of two or more elements combined in a fixed ratio
  • has characteristics different from those of its elements
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5
Q

Calcium and life

A
  • associates with calmodulin
    1) bones
    2) muscle contraction
    3) RBC development
    4) brain function –> learning and memory
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6
Q

What four elements make up 96% of living matter?

-plus calcium

A

1) Oxygen (65%)
2) Carbon (18.5%)
3) Hydrogen (9.5%)
4) Nitrogen (3.3%)
Calcium (1.5%)
-about 25 of 92 elements are essential to life

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7
Q

Hyperthyroidism
(goiter)
(thyroid growth)

A
  • Thyroid produces Thyroxine hormone (T3 and T4) from iodine
  • iodine deficiency causes the brain to secrete thyroid stimulating hormone (TSH)
  • TSH will cause the thyroid gland to grow and secrete (more) hormones
  • normally T3 and T4 will give negative feedback and tell the pituitary gland to slow down the production of TSH
  • can cause vision problems, heart attack
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8
Q

Pituitary Gland –> Thyroid –> Thyroxines (T3 and T4) –> growth, metabolism, body temp, vision, bone formation

A
  • pituitary gland produces TSH
  • Thyroid gland needs iodine to produce T3 and T4
  • sometimes thyroid hormone is given to help
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9
Q

an element’s properties depend on the…

A
  • structure of its atoms

- each element consists of a certain kind of atom that is different from those of other elements

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10
Q

Atom

A

the smallest unit of matter that still retains the properties of an element and are composed of even smaller parts called subatomic particles

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11
Q

Subatomic Particles

A

Neutrons, Electrons, Protons

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12
Q

Neutrons

A
  • subatomic particle that has no electrical charge

- found in the atomic nucleus

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13
Q

Electrons

A
  • subatomic particle that is negatively charged

- surround the nucleus in a “cloud”

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14
Q

Protons

A
  • subatomic particle that is positively charged

- found in the atomic nucleus

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15
Q

Atomic Number of an element

A

the number of protons and is unique to each element

  • Atoms of the various elements may occur in different 1) forms and differ in 2) their number of subatomic particles.
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16
Q

an atom’s electrons …

A

vary in the amount of (potential) energy they possess

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17
Q

Energy

A

the capacity to do work

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18
Q

Potential Energy

A

energy that matter possesses because of its location or structure

19
Q

Valence electrons

A

electrons in the outermost shell, or valance shell, and determine most of the chemical behavior of an atom

20
Q

Covalent Bond

A
  • sharing of a pair of valence electrons with two elements and form a molecule
  • polar and non polar
  • i.e. water (H2O), methane (CH4)
21
Q

the formation and function of molecules depend on …

A

chemical bonding between atoms

22
Q

Molecules

A

consists of 2 or more atoms held together by covalent bonds

23
Q

Single bond

A

sharing of one pair of valence electrons

24
Q

Double bond

A

sharing of two pairs of valence electrons

25
Q

Polar covalent bond

A

the atoms have differing electronegativities (attraction for the shared electrons)

  • share the electrons unequally (“hogs” all the electrons/energy)
  • i.e. water
26
Q

Ionic bond

A
  • atoms strip electrons away from their bonding partners

- electron transfer between two atoms create ions

27
Q

Ions

A

charged atoms

28
Q

Anion

A

negatively charged ion

29
Q

Cation

A

positively charged ion

30
Q

Nonpolar

A
  • don’t dissolve in water very well

- usually hydrophobic

31
Q

Ionic compounds

A
  • attraction between anions and cations
  • often called salts
  • i.e. sodium chloride (NaCl)
32
Q

Hydrogen bonding

A
  • weak chemical bond
  • forms when a hydrogen atom covalently bonded to one electronegative atom is also attracted to another electronegative atom
  • intermolecular interaction (between 2 distinct molecules)
  • i.e. ammonia and water
33
Q

Van der Waals Interactions

A
  • occur when transiently (temporary/short lived) positive and negative regions or “hot spots” of molecules that attract each other
  • partially positive or negative regions
  • collectively, such interactions can be strong, as between moleculres of a gecko’s toe hairs and a wall surface
  • AKA London forces
34
Q

4 types of bonds

A

1) Covalent
2) Ionic
3) Hydrogen bonds
4) Van der Waals

35
Q

Weak chemical bonds

A

reinforce the shapes of large molecules and help molecules adhere to each other

36
Q

the precise shape of a molecule is …

A

usually very important to its function in the living cell and is determined by the positions of its atoms’ valence orbitals

37
Q

Molecular Shape

A

determines how biological molecules recognize and respond to one another with specificity

38
Q

Chemical reactions

A

convert reactants to products

39
Q

Chemical equilibrium

A

is reached when the forward and reverse reaction rates are equal

40
Q

Intramolecular Interactions

A

interactions within the same molecule

41
Q

Photosynthesis

A

example of chemical reaction
- sunlight powers the conversation of CO2 and H2O –> glucose and oxygen

6 CO2+ 6 H2O –> C6H12O6 + 6 O2

42
Q

Glucose

A

C6 H12 O6

43
Q

Same structures have …

A

similar functions

i.e. endorphin and morphine

General Biology I E1 (5 decks)

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