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AP Chemistry > Atomic Theory > Flashcards

Atomic Theory Flashcards

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1
Q

Who is accredited with thinking up the law of conservation of mass?

A

Antoine Lavoisier

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2
Q

This law says that “different pure samples of the same compound always contain the same proportions of each element of mass”

A

The law of definite proportions

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3
Q

What were John Dalton’s four postulates?

A

1) Each element is composed of tiny particles called atoms
2) All atoms of a given element are identical and all atoms of different elements are different
3) Atoms are not created or destroyed in chemical reactions. They are dissociated, combined, or recombined
4) Compounds are formed when atoms of different elements combine with one another. A given compound always contains the same relative numbers and types of atoms

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4
Q

Who discovered electrons?

A

J.J Thompson

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5
Q

Who discovered a nucleus with protons in atoms?

A

Earnest B Rutherford

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6
Q

equal to the number of protons plus the number of neutrons

A

Mass number

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7
Q

The number of protons (or electrons in a neutral atom)

A

Atomic number

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8
Q

Same element with a different number of neutrons

A

Isotope

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9
Q

Isotopes of an element exhibit _________ chemical behavior

A

Identical

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10
Q

Atomic mass given in the periodic table is an _________ of all of the isotopes of that element

A

Average

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11
Q

In mass spectrometry, less deflection means a ___________ mass

A

Larger

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12
Q

What is the equation for average atomic mass?

A

(Mass# x %)+(Mass# x %) = average mass

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13
Q

What is the equation for mass percent of an element in a substance?

A

Mass % of element= (# of atoms of element)(elements atomic mass) / (formula weight of compound) x 100

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14
Q

Linear distance covered before a wave starts to repeat itself

A

Wavelength

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15
Q

A low frequency wave has a __________ wavelength

A

Higher

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16
Q

What is the formula for wavelength in its relation to frequency?

A

C=(wavelength)(v)

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17
Q

What is the constant in the formula?

A

3 x 10^8 m/s

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18
Q

Who hypotheses that the energy radiated from a heated objects is emitted in discrete units or quants

A

Max Planck

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19
Q

Plancks constant is represented as ____

A

H

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20
Q

The higher the frequency the _________ the energy

A

Higher

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21
Q

Highly intense _____________ light does not eject any electrons

A

Low frequency

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22
Q

When the __________________ is reached electrons are ejected immediately

A

Threshold frequency

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23
Q

Increasing the intensity of the light at a frequency that will cause electrons to eject results in a ____________ however all electrons share the same velocity

A

Higher ejection rate

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24
Q

Increasing the frequency of the light increases the velocity of the ejected electrons, however all ejected electrons ___________________

A

Share the same velocity

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25
Q

A beam of light is a stream if particles called _________

A

Photons

26
Q

What is Plancks equation?

A

E=hv

27
Q

State Coulomb’s law

A

The force of attraction decreases as the distance between the outermost electron and the protons increase

28
Q

The electrons that are furthest from the nucleus are partly _________ by the inner core electrons

A

Shielded

29
Q

The minimum amount of energy that is required to remove the outermost electron form an atom in its gas phase

A

First ionization energy

30
Q

Ionization energy generally __________ as you move across the periodic table

A

Increases

31
Q

Electrons contained in the inner shell

A

Inner core electrons

32
Q

Electrons contained in the outer shell

A

Valence electrons

33
Q

N=1 can hold how many subshells?

A

1

34
Q

What is the subshell n=1 can hold?

A

1s

35
Q

What subshells does n=2 contain?

A

2s and 2p

36
Q

How many electrons can subshell 2s hold?

A

2

37
Q

How many electrons can subshell 2p hold?

A

6

38
Q

How many electrons can 3s hold?

A

2

39
Q

How many electrons can 3p hold?

A

6

40
Q

How many electrons can subshell 3d hold?

A

10

41
Q

The shielding effect ___________ for each subshell that is added

A

Increases

42
Q

Electrons furthest from the nucleus have _________ potential energy

A

Higher

43
Q

According to the QM model, all electrons under the same subshell have __________ energy

A

The same

44
Q

A graphic representation of the space that and electron will occupy 90% of the time

A

Orbital

45
Q

Electrons are added to the _______ energy orbitals available

A

Lowest

46
Q

Atoms with unpaired electrons

A

Paramagnetic

47
Q

atoms with no unpaired electrons

A

Diamagnetic atoms

48
Q

The effective nuclear charge (the charge experience by an electron) is written as _______

A

Zeff

49
Q

As you go across the periodic table the atomic radius __________

A

Decreases

50
Q

Metals lose elections to form ________

A

Cations

51
Q

Non-metals fain electrons to form _________

A

Anions

52
Q

___________ share the same electronic configurations but have different radii

A

Isolectronic species

53
Q

_________ are smaller than smaller than neutral atoms

A

Cations

54
Q

________ are larger than neutral atoms

A

Anions

55
Q

It’s harder to pull electrons from a ________ subshell

A

Full

56
Q

First ionization energy generally _________ as atomic radii decrease

A

Increase

57
Q

The second ionization potential for an atoms is always __________

A

Greater

58
Q

An elements ability to attract electrons in a chemical bond

A

Electronegativity

59
Q

Electrons will spend _______ time around the more electronegative element in a chemical bond

A

More

60
Q

Electronegativity generally __________ as you move across the periodic table

A

Increases

61
Q

Electronegativity ________ as atomic radius decreases

A

Increases

62
Q

Who was the first to think about atomic theory?

A

Democritus

AP Chemistry (18 decks)

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