Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > Ch 1 - Anatomic Structure > Flashcards

Ch 1 - Anatomic Structure Flashcards

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

Where are protons found?

How do they relate to the atomic number of an element?

A

In the nucleus

Atomic number (Z) of an element is the
number of protons present!

Atomic number is the top number in the periodic table

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

Where are neutrons found?

How do they relate to atomic mass / MASS NUMBER?

A

In the nucleus

Atomic mass / MASS NUMBER (A) is the number of protons plus the number of neutrons.

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

What are isotopes?

A

An element can have a variable number of NEUTRONS.

Isotopes share the same atomic number (# of electrons) but have different mass numbers.

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

Where are electrons found?

What are some properties of electrons?

A

Electrons are in the space surrounding the nucleus.

Weigh very little (1/2000 of a proton)

Electrostatic force of attraction (eg being repelled) is far greater than the gravitational pull.

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

Energy levels based on electrons distance from the nucleus:

A 
Closer to nucleus: lower energy
Further out (in higher shells): higher energy
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What are valence electrons?

What do they determine?

A

Electrons that are in the shell furthest from the nucleus

These have the strongest interactions with the environment, and weakest interactions with the nucleus.

They determine the REACTIVITY of an atom.

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

What are anions and cations?

A

Negatively (anion) and positively (cation) charged atoms.

Happens when electrons are gained and lost

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

What is the difference between atomic MASS and atomic WEIGH?

Which one is reported on the atomic table?

A

Atomic MASS is the number of protons plus the number of neutrons. (Varies from one isotope to another)

Atomic WEIGHT is constant. It represents the WEIGHTED average of the isotopes.

ATOMIC WEIGHT is on the atomic table.

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

Why use atomic weight?

2

A

Gives the mass of the “average” atom of that element

Gives the mass of one “mole” of the element in grams.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is a “mole”?

How does it relate to atomic weight?

A

A number of things (atoms/ions/molecules) that equal to Avogadro’s number.

NA= 6.02 X 10^23

Ie:

The average carbon atom has a mass of 12 amu

6.02 X 10^23 Carbon atoms have a combined mass of 12g

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is the equation for Planck Relation?

A

Developed by Max Planck, it is the first quantum theory.

E = hf

E = energy of a quantum
h = planks constant (6.626 X 10^-34 J)
f = frequency of radiation
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What are quanta?

A

Electromagnetic radiation from matter. Quanta are the discrete bundles that it comes in.

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

What is the formula for angular momentum?

A

L = nh
2 (pi)

n = principal quantum number
h = Plancks constant

BECAUSE the only variable is the principal quantum number, the angular momentum of an electron changes in discrete amounts with respect to that number. (Increase n = increase in L)

*BOHR

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

What is the formula for energy of the electron?

A

E = _ Rh
n^2

Rh = rydberg unit of energy (2.18 X 10^-18 J/electron )

n = quantum number

As n increases, E becomes closer to zero (increases too - becomes less negative)

**BOHR

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

How does the energy of an electron change as it gets further away from the nucleus?

(Relating to the “energy of the electron” formula)

A

It’s energy INCREASES - becomes less negative.

Increasing n value

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

What are changes in quantum values like - discrete of infinite?

A

DISCRETE - only allow certain changes, in intervals.

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

What is the ground state of an atom?

What is it the opposite of?

A

The state of lowest energy
All the electrons are at the lowest possible orbitals

Opposite of an “excited state” where at least one electron is in a subshell of higher than normal energy.

18
Q

Are atoms usually in the ground state or the excited state - why?

A

Usually in the GROUND STATE

To minimize energy

When subjected to extreme heat or irradiation, may become excited.

19
Q

What do electrons do as they move from lower energy to higher energy?

A

AHED

A - absorb light
H - higher potential
E - excited
D - distant (from nucleus)

20
Q

What happens after brief period of excitation?

How does it relate to Planck’s relation?

A

The atoms will return to the ground state rapidly, causing an emission of discrete amounts of ENERGY in the form of PHOTONS.

(The energy emitted is the Planck relation formula, E = hf aka the energy of a quantum!!!)

21
Q

What is the equation for electromagnetic energy of a photon?

A

E = hc
(Wavelength)

h = Plancks constant 
c = speed of light in a vacuum (3.0 X 10^8 m/s)

The shirt yet the wavelength, the higher the electromagnetic energy.

22
Q

What is an atomic emission spectrum?

A

Each atom’s electrons can only be excited to distinct energy levels, which creates a unique atomic energy spectrum.

The spectrum is composed of light at certain frequencies. (Line spectrum)

23
Q

For a hydrogen atom, what is the emission spectrum like - name the different “series”:

A
  1. LYMAN SERIES
    From n=2 or greater to n=1
    (From really far to the first shell)
  2. BALMER SERIES
    from n=3 and greater to n=2
  3. PASCHEN SERIES
    From n=4 or greater to n=3
24
Q

Equation to calculate the energy associate with changes from one shell to another (ie creation if a photon through movement to ground state)

A

E = hc = _ Rh x 1 _ 1
(wavelength) Ni^2 Nf^2

This equation looks at initial minus final energy (the n’s)

The energy of the emitted photon corresponds to the difference in energy between the higher-energy initial state and the lower-energy final state

Positive E value = emission
Negative E value = absorption (excitement)

25
Q

What are protons, neutrons, and electrons?

What do they weigh?

A

Proton - positively charged (+1 atomic mass unit)
Electron - negative charge (weighs almost nothing)
Neutron - no charge (1 atomic mass unit)

26
Q

What is the quantum mechanical model?

A

Atoms fitness travel in defined orbits but are rather localized in ORBITALS (a region of space around the nucleus)

27
Q

Heisenberg uncertainty principle

A

It’s impossible to know both an electrons position and it’s momentum EXACTLY at the same time

28
Q

What is a quantum number?

A

4 numbers which can completely describe any electron in an atom

  1. Principal
  2. Azimuthal
  3. Magnetic
  4. Spin
29
Q

The principal quantum number (n)

A

Describes the average energy of a shell

Max # of electrons per shell:
2n^2

30
Q

The azimuthal quantum number (l)

A

Described the subshells within a given principal level of energy (s, d, p, or f)

Max number of electrons per subshell:
4l+2

31
Q

Magnetic quantum number (m_l)

A

Specifies the particular orbital within a subshell where an electron is likely to be found at any moment

Subshells:
1s - small circle 
2s - large circle 
2px - 2 small circles on x axis
2py - large circles overlap 
2pz - 2 s circles on y axis
32
Q

The spin quantum number (m_s)

A

Indicated the spin orientation (plus or minus 1/2) of an electron in an orbital

Two electrons in the same orbital must have opposite spins (“paired”)

Electrons in diff orbitals with the same spin are called “parallel” spins

33
Q

How is electron configuration annotated?

A

(Orbital)^(number electrons)

L and m values if quantum numbers combine to designate which orbital

Ie: 1s^2 2s^1 2p^2

2 electrons in 1s, 1 in 2a, and 2 in 2p

34
Q

What is the “building up” principle in terms of electrons and orbitals?

Aka Aufbau principle

A

Electrons fill from lower to higher subshells

35
Q

What is the n+l rule?

A

Can be used to rank subshells by increasing energy

The lower the sum of n+l values, the lower the energy of the subshell

If the number is the same for two, the one with the lower “n” will be of lower energy and fill with electrons first

36
Q

What is spectroscopic annotation for every subshell on the periodic table?

A

Assigning subshells s, p, d, and f to the periodic table.

(Where l is the azimuthal quantum number)
S means l=0
P means l=1
D means l=2
F means l=3

So for an element in 2p, l=1 and n=2

37
Q

What is hund’s rule?

A

Subshells with multiple orbitals (p, d and f) fill electrons so that every orbital in a subshell gets one electron before any of them get a second

38
Q

Paramagnetic materials - what are they?

A

Have unpaired electrons that align with magnetic fields, attracting it to a magnet

39
Q

dimagnetic materials - what are they?

A

Materials that have all paired electrons, which cannot easily be realigned. These are repelled by magnets

40
Q

What are valence electrons?

A

Electrons in the outer shell which are available for bonding with other atoms.

Atoms typically interact with each other to try and complete an octet in the valence shell

41
Q

Where on the periodic table are paired versus unpaired electrons ?

A

Unpaired electrons tend to be on the Left side (beginning of a block) and paired electrons on the Right (end of a block)

Reminder: paired electrons: paramagnetic. Unpaired electrons: diamagnetic

Chemistry (4 decks)

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