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Chemistry Honors > Atomic Structure Unit > Flashcards

Atomic Structure Unit Flashcards

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1
Q

What is Dalton’s atomic model?

A

Elements are composed of atoms; atoms are indestructible by normal chemical reactions. Atoms of the same element are exactly alike. In his model, there is a nucleus with protons and neutrons and electrons orbiting.

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2
Q

What does it mean to be electrostatically neutral?

A

To have a net charge of 0 (has both kinds of charge in equal amounts).

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3
Q

What are ions?

A

Particles that have net charge.

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4
Q

How was the electron discovered?

A

Thompson’s cathrode ray tubes. He determined that they were negatively charged particles.

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5
Q

What is Thompson’s atomic model?

A

The Plum Pudding Model - the electrons were like plums embedded in a positively charged “pudding”.

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6
Q

How was the mass of the electron discovered?

A

Through Robert Millikan’s oil drop experiment combined with Thompson’s data.

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7
Q

What was the gold foil experiment?

A

A piece of gold foil was hit with alpha particles, which have a positive charge. Most alpha particles went right through. This showed that the gold atoms were mostly empty space.

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8
Q

What were the expectations?

A

Alpha particles would pass through without changing direction (due to the evenly spread out positive charges). Determined the positive charges were in one region.

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9
Q

What were the observations?

A

Most of the alpha particles went straight through the gold foil. Some of the alpha particles bounced back. Some alpha particles were deflected.

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10
Q

What were the conclusions?

A

The atom is mostly space. The atom has a small, dense, positively-charged region called the nucleus.
Alpha particles and the nucleus have the same charge (positive) because the alpha particles were repelled.

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11
Q

What is the Rutherford Atomic Model?

A

The model described the atom as a tiny, dense, positively charged core called a nucleus, in which nearly all the mass is concentrated, around which electrons, circulate at some distance.

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12
Q

What are atoms composed of?

A

Protons, neutrons, and electrons.

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13
Q

What is the atomic number?

A

The number of protons in an atom of an element. it defines the atom. The number of protons is equal to the number of electrons (because atoms must be electrostatically neutral positive charges must equal negative charges).

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14
Q

What is atomic mass?

A

It is the average of the masses of the isotopes.

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15
Q

What is the mass number?

A

Protons plus the neutrons.

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16
Q

What are isotopes?

A

Atoms of the same element having different mass numbers.

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17
Q

What are atomic mass units relative mass?

A

1/12 the mass of carbon 12.

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18
Q

What is a positive ion?

A

An atom that loses electrons.

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19
Q

What is a negative ion?

A

An atom that gains electrons.

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20
Q

What is light?

A

AN electromagnetic wave/radiation.

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21
Q

What is wavelength?

A

The measurement from the crest of one wave to the crest of the next.

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22
Q

What is the greek symbol for wavelength?

A

Lambda.

23
Q

What is frequency?

A

The number of waves which pass a given point per unit of time.

24
Q

What is the relationship between frequency and wavelength?

A

Inversely proportional. As frequency increases, wavelength decreases.

25
Q

What is white light?

A

Light made up of many different colors of light. we can see these colors through diffraction grating.

26
Q

What is the visible spectrum?

A

The colors of light that we can see.

27
Q

What does each color of light correspond to?

A

A certain frequency and wavelength.

28
Q

What happens when an electric current is passed through an element in the gas phase?

A

The light of a particular color is observed. The bright line spectrum of that element can be shown by viewing that color through a prism or diffraction grating.

29
Q

Does every element have the same bright line spectrum?

A

No, it is different for every element.

30
Q

What is the Bohr Atomic Model?

A

In an atom, electrons (negatively charged) revolve around the positively charged nucleus in a definite circular path called orbits or shells. Each orbit or shell has a fixed energy and these circular orbits are known as orbital shells.

31
Q

What are the properties of electrons in an atom?

A
  • They exist in energy levels, and cannot be between them
  • The further the electron is from the nucleus, the more energy it has
  • Each energy level has a maximum number of electrons (2n^2)
  • Electrons can jump from their normal energy levels (ground state) to a higher level (excited state)
  • When they fall energy is released along w/light
    each electron has a different frequency
  • The frequencies together constitute the bright line spectrum for that element
32
Q

What is the wave mechanical model?

A

It is the most current model. It locates the electrons in orbitals.

33
Q

What is an orbital?

A

A region of space around the nucleus where an electron is likely to be found. There is a maximum of two electrons in every orbital.

34
Q

What is the energy equation?

A

E=hv
- E: energy of photon
-V: frequency
-h: planck’s constant

35
Q

What is Planck’s constant?

A

6.626 x 10^-34 Js

36
Q

What is the equation for the speed of light?

A

c = λν
- c: speed of light
- λ: wavelength
- ν: frequency

37
Q

What is the speed of light?

A

3.00 x 10^8 m/s

38
Q

What is a quanta?

A

The amount of energy needed to move from one energy level to another.

39
Q

What is a quantum leap?

A

When the atom gains energy, the electron leaps from a lower energy level to one that is further from the nucleus.

40
Q

What does Schrodinger’s equation describe?

A

The probability of finding the electron within a three dimensional region and predicts a three dimensional region around the nucleus called an atomic orbital.

41
Q

What is the Heisenberg Uncertainty Principle?

A

it is impossible to determine simultaneously both the position and velocity of an electron or any other particle (the better we know the position, the less we know it’s momentum).

42
Q

What is the principle quantum number?

A

energy level (n)

43
Q

What are S orbitals like?

A
  • spherical shape
  • 1 for every energy level
  • 2 max electrons
44
Q

What are P orbitals like?

A
  • dumbbell shaped
  • starts at the second energy level
  • has three different orientations
  • 6 max electrons per orbital
45
Q

What are D orbitals like?

A
  • start at third energy level
  • 5 different shapes/orientations
  • 10 max electrons
46
Q

What are F orbitals like?

A
  • they start at the fourth energy level
  • seven different shapes
  • 14 max electrons
47
Q

What is electron configuration?

A

The arrangement of electrons in an atom.

48
Q

Why is there overlap of the orbitals?

A

Because the lowest energy fills first.

49
Q

What is the Pauli Exclusion Principle?

A

No two electrons in an atom can have the same four quantum numbers, at most two electrons per orbital (going in different directions). Simplified: (1) no more than two electrons can occupy the same orbital and (2) two electrons in the same orbital must have opposite spins

50
Q

What is the Aufbau Principle?

A

Electrons occupy the orbitals of lowest energy first.

51
Q

What is Hund’s rule?

A

Electrons will fill an unoccupied orbital before they pair up.

52
Q

What are the exceptions in electron configuration?

A

Chromium and Copper, half filled sublevels have a lower energy (more stable).

53
Q

What is the order of electron configuration?

A

1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p

Chemistry Honors (11 decks)

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