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MCAT chemistry > Chapter 1 > Flashcards

Chapter 1 Flashcards

1
Q

What is all matter composed of?

A

atoms which are subatomic particles

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2
Q

protons carry what charge and have what mass?

A

+1 charge and have a mass of 1 amu/ 1 Da actual charge is 1.6 x 10-19 C

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3
Q

Neutrons have what charge and what mass

A

neutral and 1 amu

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4
Q

protons and neutrons can be called what?

A

nucleons

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5
Q

electrons have what charge and mass

A

-1 charge and negligible mass actual charge is -1.6 x 10-19 C

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6
Q

What is the atomic number (Z)

A

the number of protons of the atom and gives the element its unique identity

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7
Q

What is the mass number (A)

A

the total number of neutrons and protons contained in the nucleus

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8
Q

what is an isotope

A

atoms of the same element that have different numbers of neutrons

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9
Q

What is Deuterium (D or 2H)

A

An isotope of (1H that has no neutrons) that has one proton and one neutron

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10
Q

what is a cation

A

ions that carry a net positive charge

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11
Q

what is an anion

A

ions that carry a net negative charge

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12
Q

polyatomic ions that have positive charges

A
  • represented by roman numerals - the ion with lesser charge uses suffix -ous - the ion with greater charge use suffix -ic
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13
Q

polyatomic ions with oxygen

A
  • use suffix -ite for fewer oxygens - use suffix -ate for more oxygen atoms
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14
Q

polyatomic ions with hydrogen

A
  • one hydrogen is hydrogen (atom name) - two hydrogens is dihydrogen (atom name)
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15
Q

Bohr model of the hydrogen atom:

A

electrons orbit the nucleus in spherical shells

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16
Q

Electrons closest to the nucleus…

A

experience the greatest attractive force so it has greater stability and lower energy level

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17
Q

electrons furthest from the nucleus…

A

have a higher energy level and be less stable

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18
Q

what is the ground state

A

the lowest possible energy level closest to the nucleus

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19
Q

when is an electron excited

A

when it absorbs energy equal to the difference between a higher shell’s energy level and the ground states energy level and jumps to the higher-energy shell

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20
Q

when an electron jumps back down to ground state?

A

energy is emitted in the form of a photon

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21
Q

energy is admitted and absorbed in the form of

A

electromagnetic radiation

22
Q

the energy of electromagnetic radiation formula is

A

E=hf (h = Plank’s constant 6.63 x 10-34 J) (f = frequency of light)

23
Q

E=hf can also be described as…

A

E = hc/ wavelength (h = Plank’s constant 6.63 x 10-34 J) (c = speed of light 3.00 x 108 m/s is a vacuum)

24
Q

equation to calculate the energy level held by an electron at a certain energy level

A

E = -(R/n2) R = Rydberg constant 2.18 x10-18 J) n = energy level at which the electron is present

25
Q

Rydberg formula determines the energy level and wavelength of the emitted or absorbed radiation as an electron moves

A

deltaE=hc/wavelength= R(1/nf2 - 1/ni2) R = Rydberg constant 2.18 x10-18 J) n = energy level at which the electron is present

26
Q

Moving from a higher to a lower energy level is associated with

A

emission

27
Q

moving from a lower level to a higher one

A

requires energy absorption

28
Q

Heisenberg uncertainty principle

A

posits that the more we know about the position of an electron, the less we know about its momentum and vice versa (cannot know both position and momentum of an electron at the same time)

29
Q

system of quantum numbers

A

helps describe electrons to an extent

30
Q

electrons exist in?

A

orbitals (areas of space where electrons are likely to be located)

31
Q

each orbital can hold how many electrons

A

max of 2

32
Q

principal quantum number (n)

A

the energy level of the electron (1 or greater) - relates to the row of the table in which the element is found

33
Q

azimuthal or angular momentum quantum number (l)

A

describes the sub shell of the principal quantum number where the electron is found and range from 0 to n - 1 l = 0 is the s subshell l = 1 is the p subshell l = 2 is the d subshell l = 3 is the f subshell

34
Q

magnetic quantum number (ml)

A

describes the spatial orientation of the orbital in question within its subshell l = 0 holds one orbital l = 1 holds 3 orbitals l = 2 holds 5 orbitals l = 3 holds 7 orbitals

35
Q

spin quantum number (ms)

A

describes the spin orientation of the electron which relates to its angular momentum -1/2 or +1/2 2 electrons in same orbital have opposite spin

36
Q

electron configuration

A

describes the arrangement of electrons in sub shells around the atomic nucleus ex. A 3d subshell that contains 8 electrons would be denoted as 3d8

37
Q

Aufbau principle

A

electrons fill lower-energy orbitals first to create the most stable electron configuration

38
Q

Hund’s rule

A

each electron would rather exist in an orbital by itself if possible so we fill each half way first then fill

39
Q

Element blocks of the periodic table

A
40
Q

valence electrons are

A

the electrons furthest away from the nucleus

41
Q

periods are also known as

columns are also known as

A
  1. rows
  2. families
42
Q

division of the periodic table

A
43
Q

effective nuclear charge (Zeff)

A

the attractive force of the nucleus on the atom’s valence electrons

as number of protons increases from left to right, Zeff also increases but moving down the table Zeff decreases

44
Q

atomic size or radius

A

inversely related to Zeff so as we go from left to right, atomic size decreases but as we go down, it increases

45
Q

ionic radius (the radius of a charged speices)

A

ionic radius of a cation is smaller than the ionic radisu of an anion in comparison to an uncharged form

46
Q

ionization energy

A

the energy required to move one valence electron from a neutral atom in a gaseous state

positive value

the first ionization energy is always smaller than the second

directly related to Zeff so it increases from left to right and decreases as we go down columns

47
Q

electron affinity

A

denotes the amount of energy released when an electron is added to an atom

atoms that can more readily accept an electron, such as holegns have higher electron affinities.

Directly related to Zeff so increases from L to R and decreases from up to down

exception is noble gases because they posess stable octet

48
Q

electronegativity

A

the tendency of an atom to attract electrons that are shared in a chemical bond between 2 atoms

direclty related to Zeff, increases from L to R and decreases from up to down

49
Q

difference between electron affinity and electronegativity

A

electronegativity direclty relates to behaviour within a chemical bond

50
Q

trends summarized

A

all related to Zeff except atomic size/radius

MCAT chemistry (12 decks)

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