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Chemistry AP > Structure Of The Atom > Flashcards

Structure Of The Atom Flashcards

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0
Q

Law of constant composition and who discovered it

A

Each pure chemical compound always has the same percentage composition of each element by mass - Joseph Proust

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1
Q

Law of conservation of matter and who discovered it

A

Matter cannot be destroyed or created in a closed system - Andrew Lavoisier

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2
Q

Atomic Theory and who discovered it

A
  1. All matter is composed of atoms that cannot be destroyed or created
  2. Each element has atoms that identical to each other in all of their properties and these properties are different from all other atoms
  3. Chemical reactions are rearrangements of atoms in small whole-number ratios
    - John Dalton
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3
Q

What did Michael Faraday do?

A

Showed electric current could cause chemical reactions

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4
Q

What did William Crookes do?

A

Developed the cathode ray tube

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5
Q

What did J. J. Thompson do?

A

Determined cathode rays were fundamental parts of electrons

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6
Q

What did Robert Millikan do?

A

Calculated the charge of an electron using his oil drop experiment

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7
Q

What is the “plum pudding” model of the atom?

A

Electrons are bathed in a sea of positive charges

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8
Q

What did Ernest Rutherford do?

A

Gold foil experiment and determined the nuclear model of the atom
Also discovered the proton

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9
Q

What is Heisenberg’s uncertainty principle?

A

The position and momentum of any particle cannot both be known at the same time

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10
Q

Ground state

A

Lowest possible energy state of an atom

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11
Q

Excited state

A

When an atom has more energy than ground state

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12
Q

What is the formula to calculate wavelength or frequency

A

(Wavelength)(frequency)=speed of light(3.0 x 10^8

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13
Q

What is h?

A

Planck’s constant, proportionality constant

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14
Q

How do you calculate energy?

A

E=hv=(hc)/λ

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15
Q

What happens when energy moves from a higher number orbit to a lower number orbit?

A

Energy is emitted

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16
Q

What does an electron need to move to a higher numbered orbit?

A

Energy

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17
Q

What is the relationship between momentum of an electron and its orbit size?

A

mv=(nh)/(2πr)

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18
Q

What is Bohr’s radius?

A

σ = 53 pm

19
Q

Who suggested that electrons could behave like a wave as well as a particle?

A

Louis de Broglie

20
Q

What is the equation for wave-particle duality?

A

(hc)/λ = hv = mc^2

21
Q

What is the uncertainty equation?

A

(Δx)(Δmv) <= h/4π

22
Q

What does the value n represent?

A

The number of the principal energy level

23
Q

Where are sublevels located?

A

Within each principal energy level

24
Q

How many sublevels are possible for each principle energy level?

A

Equal to the value of n

25
Q

What four letters are also given to sublevels?

A

s, p, d, and f

26
Q

Where are orbitals located?

A

Within sublevels

27
Q

What are orbitals?

A

Regions of space that have high electron density

28
Q

What number of orbitals can a sublevel have?

A

2l + 1

29
Q

What shape are s sublevels?

A

Spherical

30
Q

What shape are p sublevels and how many orientations are there?

A

Dumbbell shaped, 3 orientations

31
Q

What shape are d orbitals and how many orientations are there?

A

X shaped, 5 orientations

32
Q

How do you describe electrons in every atom?

A

Electron configuration

33
Q

How are the electrons present in an atom listed?

A

nl^x

34
Q

What is the aufbau?

A

Energy order

35
Q

Which elements don’t follow aufbau ordering?

A

Cr, Mo, Cu, Ag, and Au

36
Q

What are valence electrons?

A

The outermost electrons of an atom - only s and p electrons

37
Q

What is Hund’s Rule?

A

p, d, and f orbitals in a sublevel must all be filled with one electron each before a second electron is allowed to pair in any orbital

38
Q

What is the purpose of quantum numbers?

A

To describe each electron in an atom

39
Q

What does the principal quantum number (n) represent? What values can it have?

A

The principal energy level of the atom - can be any integer value from 1 or higher

40
Q

What does the azimuthal quantum number (l) represent? What are its possible values?

A

Designates the sublevel if the electron and represents the shape of the orbitals - can be 0 - (n-1)

41
Q

What does the magnetic quantum number (ml) represent? What are its possible values?

A

Designates the orientation of the orbital - can be from -l to +l

42
Q

What does the spin quantum number (ms) represent? What are its possible values?

A

Represents the spin of the electron - can be +1/2 or -1/2

43
Q

What is the Pauli exclusion principle?

A

No two electrons in the same atom may have the same 4 quantum numbers

44
Q

What order are quantum numbers written?

A

n, l, ml, ms

Chemistry AP (2 decks)

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