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My MCAT > Atomic Structure & Periodic Trends > Flashcards

Atomic Structure & Periodic Trends Flashcards

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MCAT flashcards
1
Q

What is the Molarity (M) formula?

A

moles of solute/liters of solution = mol/L

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2
Q

What is the molality (m) formula?

A

moles of solute/kilograms of solvent = mol/kg

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3
Q

What is electronegativity?

A

the tendency for an atom to attract a bonding pair of electrons. Electronegativity unlike other periodic trends is measured within a bond.

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4
Q

What does Zeff stand for?

A

Effective nuclear charge

Zeff is the net positive charge pulling these electrons towards the nucleus. The stronger the pull on the outermost electrons (valence electrons) towards the nucleus, the higher the effective nuclear charge.

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5
Q

What is the effect of Zeff on periodic trends?

What does higher Zeff correlate with on the periodic table?

A

The greater the effective nuclear charge the greater the electronegativity

Effective nuclear charge depends on the number of protons in the nucleus, the distance from the nucleus, and the amount of shielding by inner shell electrons. The number of protons increases Zeff​ , while the distance and amount of shielding decreases Zeff​

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6
Q

True or False: Zeff depends on the attraction of the bonding pair towards the nucleus

A

False

Effective nuclear charge depends on the number of protons in the nucleus, the distance from the nucleus, and the amount of shielding by inner shell electrons. The number of protons increases Zeff​ , while the distance and amount of shielding decreases Zeff​

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7
Q

The atomic number is represented by the letter…

A

Z

the # of protons = Z

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8
Q

The mass number is represented by the letter…

A

A

the # of protons + neutrons = A

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9
Q

Group 1 of the periodic table is…

A

alkali metals

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10
Q

What are characteristics of alkali metals?

A
  • distinctive flame colors
  • good electrical conductors
  • solid under standard conditions
  • shiny or lustrous
  • ductile (can be easily stretched into wires)
  • malleable (can be made into shapes/sheets)
  • very reactive!

mercury is the exception to the solidity characteristic

alkali metals have lone valence electrons making them incredibly reactive

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11
Q

Group 2 of the periodic table

A

Alkaline earth metals

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12
Q

What are characteristics of alkaline earth metals?

A
  • metallic character
  • reactive
  • good conductors
  • oxidation state of 2+

they also form hydroxides when they react with water

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13
Q

What are characteristics of transition metals?

A
  • lusterous
  • hard & durable
  • good conductors
  • take on vivid colors due to electronic transitions between D orbitals
  • multiple oxidation states

characterized by many oxidation states due to the low reactivity of the unpaired d electrons

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14
Q

What are characteristics of non-metals?

A
  • not shiny/lustrous
  • poor conductors
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15
Q

What are the characteristics of metalloids

also known as semimetals

A

they share the characteristics of metals and non-metals
* brittle
* poor to decent conductors
* act like nonmetals in chemical reactions, but can vary

Boron and Silicon are the ones you will most likely see on the MCAT

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16
Q

Chalcogens are

what group #? What elements?

A

Group 16, include oxygen and sulfur

have nearly filled valence shells

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17
Q

What is group 17 of the periodic table?

A

Halogens

F, Cl, Br, I

have nearly filled valence shells and are very reactive, especially with alkali metals

18
Q

What is the effect of Zeff on periodic trends?

What does higher Zeff correlate with on the periodic table?

A

The greater the effective nuclear charge the greater the electronegativity

Effective nuclear charge depends on the number of protons in the nucleus, the distance from the nucleus, and the amount of shielding by inner shell electrons. The number of protons increases Zeff​ , while the distance and amount of shielding decreases Zeff​

19
Q

Describe the relationship between transition metals and ionization energy

A

transition metals have little variability in their ionization energies and electronegativities due to their similar valence electron shells, which is the s shell

20
Q

What is the relationship between reactivity and oxidation states

A

High reactivity would limits the number of oxidation states

21
Q

The amount of energy required to remove an electron from an isolated atom or molecule is….

A

ionization energy

22
Q

the energy change that results from adding an electron to a gaseous atom

A

electron affinity

23
Q

What periodic aligns with the radius of an atom decreasing from left to right across a period as more protons and electrons are added?

A

atomic radius (also called atomic size)

24
Q

______, _____ and _____ periodic trends increase diagonally from bottom left to top right

A

Ionization energy, electron affinity, and electronegativity

25
Q

E = hf represents …

What does each variable stand for? What does the equation quantify?

A

Electromagnetic radiation

E = energy of electromagnetic radiation
h = Plank’s constant
f = frequency of light

26
Q

What are the units of the frequency of light (f) ?

A

3.00 x 108 m/s

27
Q

True or False

Electromagnetic radiation includes the full continuum of light

A

True!

This radiation encapsulates full continuum of wavelengths

Think of everything from visible light to gamma waves to X-rays!

28
Q

E = hc/ƛ represents….

What does it quantify? What do the variables represent?

A

The energy of a photon

This equation is equal to the electromagnetic radiation formula E=hf !

29
Q

True or false

Each element has an absorption and emission sprectrum

A

True!

Since energy is aborrbed and released in quanta, the absorption or emission of electromagnetic radiation results in a caracteristic absorption and emission spectrum that are unique for each element

30
Q

Name the equation

What does it represent?

A

The Rydberg formula

Used to predict the wavelength of light resulting from an electron moving between energy levels of an atom

31
Q

What does this equation represent?

Eqn 4. pg. 6 NS

A

Energy change (in Joules) of an electron moving between energy levels

Modified Rydberg equation

32
Q

(+) ΔE means that energy is ____ and - ΔE means that energy is _____

A

absorbed, released

33
Q

Define the term

Posits that we cannot simultaneously know the exact position and the momentum of a given electron

A

Heisenberg uncertainty principle

34
Q

Denotes the energy level of an electron

Corresponds to the Bohr radii

Hint: represented by n

A

principle quantum number

the higher the n value, the greater the energy, and thus the further the distance from the nucleus

35
Q

The periodic table is arranged in rows corresponding to…

A

Bohr radii; n

i.e Sodium is in the 3rd period, and this element has a principal quantum number of n=3

36
Q

What quantum number describes the shape of an orbital’s subshell?

Give the letter and the name

A

angular momentum quantum number (l)

azithmul quantum number

note: there is 1 s orbital, 3 p orbitals, 5 d orbitals, and 7 f orbitals

37
Q

Which quantum number describes the spatial orientation of the orbital region of space with respect to an applied magnetic field?

A

magnetic quantum number ml

described in integers of -l to +l

38
Q

What quantum number describes the spin orientation of the electron in an external magnetic field?

A

spin quantum number ms

the two spin orientations are ms = +1/2 (up) or -1/2 (down). Note that because of spin orientations, an s orbital can have up to 2 electrons, p orbitals 6 electrons, d can have 10, and f can have 14

39
Q

Name the principle/rule:

every orbital in a sublevel is singly occupied before any orbital is doubly occupied

A

Hund’s rule

40
Q

Name the principle/rule:

electrons are filled into atomic orbitals in the increasing order of orbital energy level

A

Aufbau principle

41
Q

Name the principle/rule:

No two electrons can have the same quantum numbers

A

Pauli exclusion principle

My MCAT (30 decks)

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