Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

CHEM/OCHEM (MCAT) > Intro to General Chemistry > Flashcards

Intro to General Chemistry Flashcards

You may prefer our related Brainscape-certified flashcards:
MCAT flashcards AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

Which of the following particles form the nucleus of the atom? Select all that apply.

a) proton
b) neutron
c) electron

A

proton and neutron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is the approximate mass of a proton?

a) 1 amu
b) 0 amu

A

mass of proton = 1 amu

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is the approximate mass of an electron?

a) 1 amu
b) 0 amu

A

mass of electron = 0 amu

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is the approximate mass of a neutron?

a) 1 amu
b) 0 amu

A

mass of neutron = 1 amu

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is the atomic number and what is the single letter abbreviation for it?

A

number of protons

Z

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is the mass number? What is its single letter abbreviation?

A

number of protons + neutrons

A

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What are isotopes?

A

elements that have the SAME number of PROTONS but DIFFERENT number of NEUTRONS

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

TRUE or FALSE: Elements of the same period are most likely to react in similar ways.

A

FALSE –> Elements of the same GROUP are most likely to react in similar ways

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What are the 4 quantum numbers and what do they describe?

A 
n = principle quantum number --> energy level and distance from nucleus
l = angular momentum quantum number --> orbital shape (s, p, d, f)
ml = magnetic quantum number --> orbital orientation (px, py, pz)
ms = spin quantum number --> spin of the electron
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What are the possible values for each of the quantum numbers?

A 
n = 1, 2, 3, ...
l = n-1
ml = -l to +l (e.g. 3 ml values for l  = 1)
ms = +1/2 (up) or -1/2 (down)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What are the orbital shapes (spdf) for the following l values? What are the n values?

l = 0
l = 1
l = 2
A 
l = 0 --> s --> n = 1
l = 1 --> p --> n = 2
l = 2 --> d --> n = 3
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is the Aufbau principle?

A

electrons occupy lowest energy level first (e.g. 1s before 2s)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is Hund’s rule?

A

electrons will fill all subshells SINGLY before pairing up

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is the Pauli Exclusion Principle?

A

no 2 electrons in an atom can have the same set of quantum numbers

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What is the spdf notation for carbon (C)? Provide both full and abbreviated forms.

A

full –> 1s^2 2s^2 2p^2

abbreviated –> [He] 2s^2 2p^2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

TRUE or FALSE: electrons always lose the outer most (highest n) electrons first.

A

TRUE

e.g. Co loses one electron…

Co = [Ar] 4s^2 3d^7 –> Co = [Ar] 4s^1 3d^7 [CORRECT]

Co = [Ar] 4s^2 3d^7 –> Co = [Ar] 4s^2 3d^6 [WRONG]

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

TRUE or FALSE: Electrons can move to different energy levels to fill orbitals in such a way that subshells are half-filled or completely filled.

A

TRUE –> Half-filled or completely filled subshells are more stable.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What does diamagnetic mean in terms of electron configuration?

A

all electrons are paired up –> magnetic fields cancel (no net magnetic field)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What does paramagnetic mean in terms of electron configuration?

A

unpaired electrons present –> NET magnetic field

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Metals ___a___ electrons and form _____b_____ to obtain noble gas configuration.

a) lose/gain
b) cation/anion

A

metals lose electrons –> form cations

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Non-metals ___a___ electrons and form _____b_____ to obtain noble gas configuration.

a) lose/gain
b) cation/anion

A

non-metals gain electrons –> form anions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

An ionic bond forms between a/an _____________ and a/an ______________.

A

metal and non-metal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

A covalent bond forms between a/an _____________ and a/an ______________.

A

non-metal and non-metal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What is the most electronegative atom on the periodic table?

A

Fluorine

Remember: F O N Cl –> uncle FONCl lol

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Why is a cation smaller than an anion?

A

cation LOSES electrons
anions GAIN electrons

(Remember: if asked about isoelectronic species, the atom with an OVERALL NEGATIVE charge is the largest)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

What is lattice energy?

A

amount of energy required to break apart an ionic lattice

27
Q

Which rule takes priority in determining greater lattice energy?

a) greater charge
b) smaller radius

A

a) greater charge

28
Q

What is ionization energy?

A

minimum energy required to completely remove an electron from a neutral gaseous atom

29
Q

TRUE or FALSE: First ionization energy is always greater than the second ionization energy.

A

FALSE –> 2nd ionization energy is always GREATER

30
Q

Of the nonradioactive elements, which element has the largest first ionization energy?

a) chlorine
b) fluorine
c) helium
d) neon

A

c) helium

hint: consider periodic trends

31
Q

Why is electron affinity always positive for noble gases?

A

noble gases are stable and REQUIRE energy (endothermic) to gain an electron

32
Q

Given the velocity and wavelength, what is the formula for frequency?

A

frequency = velocity / wavelength

33
Q

TRUE or FALSE: In electromagnetic radiation (EMR), electric and magnetic fields are created parallel to each other and the direction of travel.

A

FALSE: they are PERPENDICULAR

34
Q

When EMR (electromagnetic radiation) waves travel in a vacuum, what is its velocity equal to?

A

speed of light

35
Q

What is the value for the speed of light?

A

c = 3 x 10^8 m/s

36
Q

What is Planck’s equation?

A

E = hf = hc/wavelength

37
Q

TRUE or FALSE: short wavelengths are more dangerous than long wavelengths.

A

TRUE

38
Q

What is the difference between absorption line spectrum and emission line spectrum?

A

absorption –> dark lines on light background

emission –> light lines on dark background

39
Q

What is deBroglie’s postulate? Provide the formula.

A

wavelength = h/p = h/(mv)

note: h = Planck’s constant, p = momentum

40
Q

What does the Heisenberg Uncertainty Principle state?

A

exact position and momentum cannot be measured simultaneously

41
Q

What did the photoelectric effect (experiment) demonstrate?

A

particle nature of light

42
Q

Which of the following are intramolecular bonds? Select all that apply.

a) metallic
b) covalent
c) hydrogen bonding
d) London dispersion forces
e) ionic
f) dipole-dipole

A

a) metallic
b) covalent
e) ionic

43
Q

What are the 3 electronegative atoms that can form a hydrogen bond?

A

F O N

44
Q

How man hydrogen bonds can one molecule of water form?

A

4

45
Q

TRUE or FALSE: molecules that possess an O, N, or F can form hydrogen bonds, yielding low melting and boiling points

A

FALSE: O, N, F –> HIGH bp and mp

46
Q

As the number of INTERmolecular forces between molecules ______a______, the boiling point and melting point ______b______.

a) increase/decrease
b) increase/decrease

A

a) increase
b) increase

or a) decrease b) decrease

47
Q

List the following from strongest to weakest…use equal sign if equivalent:

dipole-dipole
ionic
H bonding
covalent
metallic
London dispersion
A

ionic = covalent = metallic > H-bonding > dipole-dipole > London dispersion

48
Q

What particle(s) is/are emitted/broken down in alpha decay?

A

alpha particle (2 protons and 2 neutrons) released

alpha particle = superscript 4, subscript 2, He2+

49
Q

What particle(s) is/are emitted/broken down in negative beta decay?

A

neutron –> proton and electron

note: the electron is known as the beta particle

50
Q

What particle(s) is/are emitted/broken down in gamma decay?

A

excited nucleus relaxes (energy released)–> gamma rays (high energy photons)

51
Q

Which type of radioactive decay is most dangerous?

a) alpha decay
b) beta decay
c) gamma decay

A

c) gamma decay

52
Q

Define a half-life.

A

A half-life is the time it takes for half a given sample to decay.

53
Q

TRUE or FALSE: the half-life of radioactive decay is dependent on time.

A

FALSE: half-life of radioactive decay is INDEPENDENT of time.

54
Q

is Mg more or less electronegative than Na

A

more

55
Q

does electronegativity increase to the left or right of the periodic table

A

to the right

56
Q

if there are more stuff protons, there is ____ of electrons

no shielding or more shielding

A

more shielding

57
Q

what is the periodic trend for increasing protons

A

going from top to bottom, the number of protons increases

58
Q

what is the Zeff periodic trend and how does it work

A

it increases downwards and to the right
the more protons there are, the more positive charge acting on the valence electrons, increasing Zeff
the less protons there are, the less positive charge acting on the valence electrons, decreasing Zeff

59
Q

atomic radius increases from _____ to _____ and from ____ to _____

bottom/top
right/left

A

top to bottom and right to left

60
Q

if an atom has more protons than electrons, the size will be greater - true or false, if false, why

A

false - the size will be smaller because the more protons there are, the greater the electrons will be pulled in, thus the atom will become tighter and smaller

61
Q

is K + greater in size than Cl- , why or why not

A

no, because Cl- has fewer protons which mean there is less electron attraction to pull it in smaller

62
Q

what is the ionization energy periodic trend

A

it increases to the right and from bottom to top

63
Q

what is electron affinity

A

the element’s attraction for electrons

64
Q

why does Chlorine have a larger electron affinity than potassium

A

because chlorine needs only one more electron to achieve a full shell, so it has a greater want for the electrons than potassium which would rather lose an electron

CHEM/OCHEM (MCAT) (10 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions