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cell and molecular biology > atoms and elements > Flashcards

atoms and elements Flashcards

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AP® Biology flashcards Biology 101 flashcards
1
Q

what is an atom

A

an atom is the smallest unit of matter but still has the properties of an element

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2
Q

what is an atom made of

A

3 sub-atomic particles called protons, neutrons and electrons

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3
Q

what is the charge of protons, neutrons and electrons

A

protons +1, neutrons 0, electrons -1

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4
Q

what is the mass of protons, neutrons, electrons

A

protons 1, neutrons 1, electrons 1/1837

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5
Q

where are protons, neutrons and electrons located

A

protons and neutrons are in the nucleus and electrons surround the nucleus

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6
Q

what is another unit for atomic mass unit (amu)

A

dalton

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7
Q

describe the mass of protons and neutrons

A

they have an identical mass of 1.7x10-24 g

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8
Q

what is the mass of a proton and neutron

A

1 dalton

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9
Q

what are the two models called

A

planetary model (bohr model) and electron cloud model schrodinger

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10
Q

when was the planetary model made

A

1913

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11
Q

when was the electron cloud model made

A

1926

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12
Q

describe the electron cloud model

A

represents the two electrons as a cloud of negative charge

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13
Q

describe the planetary model

A

the electrons are shown as two spheres on a circle around the nucleus

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14
Q

what is mass number

A

number of protons + number of neutrons

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15
Q

what does a proton determine

A

an element

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16
Q

what does a neutron determine

A

an isotope

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17
Q

what is an isotope

A

a different atomic form of the same element but with different number of neutrons but same number of protons

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18
Q

what is ground state

A

when the distance between the electron and proton is smaller (than excited state)

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19
Q

what is the excited state

A

when the distance between the electron and proton is larger (than ground state)

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20
Q

what is the atomic number

A

sum of protons

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21
Q

what is an element

A

a substance that can’t be broken down to any other substances by chemical reactions

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22
Q

what is sodium used for

A

salt, streetlights, in our bodies (for muscles)

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23
Q

what is chlorine used for

A

toxic gas, water treatment, pvc (plastic)

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24
Q

what is a compound

A

a substance that consists of two or more different elements combined

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25
Q

what is an example of a compound

A

water ( 2H2 + O2= 2H2O)

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26
Q

is the atomic number the bottom or top number

A

top number

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27
Q

is the atomic mass the bottom of top number

A

bottom number

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28
Q

what is an example of an isotope

A

carbon= 12C (6 protons), 13C (7 p) and 14C (8 p)

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29
Q

do isotopes behave the same or different in chemical reactions

A

the same

30
Q

why are 12C and 13 C (isotopes) more stable than 14C

A

because the more neutrons you have the more unstable and radioactive the isotope

31
Q

what happens to the stability and radioactivity of the isotope when the number of neutrons increases

A

stability decreases and radioactivity increases

32
Q

what is a radioactive isotope

A

when a nucleus decays spontaneously which gives off energy and particles

33
Q

what is radioactive decay

A

a change in the number of protons

34
Q

what does radioactive decay cause

A

causes the atom to transform into an atom of a different element

35
Q

are atomic masses always whole numbers

A

no they may be integers

36
Q

what is the atomic mass of isotopes

A

the average of the different isotopes

37
Q

what are the types of radioactive decay

A
  • alpha decay
  • beta decay
  • gamma decay
38
Q

what is alpha decay

A

is when the nucleus loses 2 protons

39
Q

what is beta decay

A

when the nucleus either loses or gains a proton

40
Q

what is gamma decay

A

when the number of protons doesn’t change so there isn’t a change in element

41
Q

what can radioactive isotopes be used as in medicine

A

diagnostic tools

42
Q

what are radioactive tracers

A

they are radioactive isotopes that are combined into biologically active molecules which are then used to track atoms during metabolism

43
Q

what are radioactive tracers also combined with

A

PET scanners to monitor growth and metabolism of cancers

44
Q

what happens with energy as we move further away from the nucleus

A

energy increases

45
Q

describe the energy of the outer shell

A

has the highest energy

46
Q

describe the reactivity of an atom with full shell

A

unreactive

47
Q

what is valence

A
  • bonding capacity of an atom
  • number of covalent bonds the atom can form (equal to number of unpaired electrons on outer shell)
48
Q

what is valence electron

A

an electron in outer shell

49
Q

what’s valence shell

A

the outer shell with most energy and with valence electron

50
Q

what are 3 ways of showing electron configuration

A
  • electron distribution diagram
  • superimposed orbitals
  • separate electron orbitals
51
Q

what is chemical behaviour based on

A

the number of electrons on it’s outer shell

52
Q

describe the chemical beh of atoms with same number of outer electrons

A

similar chemical behaviour

53
Q

what are types of bonds

A
  • covalent bonds
  • ionic bonds
  • electronegativity
54
Q

what is a covalent bond

A
  • a shared pair of electrons
  • strongest bond
55
Q

what are examples of covalent bonds

A
  • hydrogen
  • oxygen
    -water
    -methane
56
Q

what is electronegativity

A

attraction of an atom to electrons of a covalent bond

57
Q

what is a non-polar covalent bond

A

a covalent bond where the two atoms have similar electronegativity

58
Q

what is a polar covalent bond

A

a covalent bond between atoms that have different electronegativity

59
Q

what happens to the electrons in a polar covalent bond

A

the electrons are pulled closer to the more electronegative atom (delta negative and other delta positive)

60
Q

what is an ion

A

an atom that has gained or lost an electron so has gained a charge

61
Q

what is a cation

A

a positively charged ion (lost an electron)

62
Q

what is an anion

A

a negatively charged ion (gained an electron)

63
Q

what is an ionic bond

A

a chemical bond from an attraction between oppositely charged ions

64
Q

name weak chemical interactions

A
  • hydrogen bonds
  • van der walls
65
Q

what is a hydrogen bond

A

a weak chemical bond where a partially positive hydrogen atom is attracted to a partially negative hydrogen atom from a different polar bond

66
Q

when was van der waals discovered

A

1873

67
Q

where do van der walls exist

A

solids, liquids, gases

68
Q

what are the tree types of van der waals

A
  • dipole induced dipole
  • dipole dipole (strongest type)
  • london dispersion forces
69
Q

what is a dipole

A

a set of separated charges in an atom

70
Q

what is a dipole dipole

A

is an attraction between 2 polar molecules

71
Q

what is a dipole induced dipole

A

an attraction between a polar molecule and an atom with an induced dipole

72
Q

what is a london dispersion force

A

an attraction between a nonpolar atom with an instantaneous dipole and a nonpolar atom with an induced dipole

cell and molecular biology (7 decks)

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