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DAT GenChem > GenChem1 (AtomStructure) > Flashcards

GenChem1 (AtomStructure) Flashcards

1
Q

Electrons exist outside the nucleus in characteristic regions of space called

A

orbitals

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2
Q

All atoms of an element cannot be broken down further by ________ means

A

chemical

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3
Q

What is the mass of 1 proton?

A

1 amu

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4
Q

Z represents what aspect of an element?

A

Atomic number

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5
Q

What is the atomic number of an element?

A

The # of protons

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6
Q

All atoms of a given element have the same

A

Atomic number

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7
Q

What is the mass of one neutron?

A

Slightly more than 1amu (more than a proton)

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8
Q

What is the mass number of an atom?

A

The # of protons + neutrons

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9
Q

A represents what aspect of an element?

A

Mass number

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10
Q

The electrons furthest from the nucleus are known as

A

Valence Electrons

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11
Q

The farther electrons are from the nucleus, the STRONG/WEAKER the attractive force of the positively charged nucleus is?

A

Weaker

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12
Q

Generally speaking, what determines the reactivity of an atom?

A

Valence electrons

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13
Q

Determine the number of protons. neutrons, and electrons in a Nickel-58 atom and a Nickel 60 2+ cation?

The atomic number of Nickel is 58

A

Nickel 58 –> 28 protons, 28 electrons, 30 neutrons

Nickel 60 2+ –> 28 protons, 26 electrons, 32 neutrons

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14
Q

The atomic mass of an atom is the relative mass of that atom compared to the mass of a…

What is the standard assigned mass of it?

A

Carbon-12 atom

12.000amu

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15
Q

One amu is one twelfth the mass of the carbon 12 atom, approximately

A

1.66*10^-24 (g)

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16
Q

Atomic weight is the….

A

weight of an atom in grams per mole

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17
Q

One mole is equal to how many particles?

A

6.022*10^23 particles

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18
Q

6.022*10^23 carbon atoms weighs

A

12.0g

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19
Q

What is an isotope

A

Atoms with the same number of protons but different numbers of neutrons

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20
Q

Are the chemical properties of isotopes similar to the non-isotope form? Why?

A

Yes. They have the same number of protons and electrons.

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21
Q

The energy value of a quantum (E) is equal to…

A

hf

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22
Q

h =

A

6.62610^-34 Js

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23
Q

Bohr’s model, based upon Rutherford’s findings, assumed that in the hydrogen atom there was a central proton around which an electron traveled in what type of motion?

A

Circular Orbit

24
Q

What is the equation for angular momentum in Bohr’s theory?

A

nh/2π

25
Q

Bohr equated the allowed values of angular momentum to the energy of the electron and got what equation?

A

E= - R(H)/n^2

Energy of the electron changes in discrete amounts with respect to the quantum number!

26
Q

R(H) =

A

2.18*10^-18 J/electron

27
Q

A smaller radius means higher or lower energy state of an electron?

What is the lowest energy state of an electron called (n=1)

A

Lower

Ground State

28
Q

The electromagnetic energy of emitted photons from an atom returning to the ground state from an excited state is…

A

E=hc/λ

29
Q

Each element can have its electrons excited to distinct energy levels, so each atom possesses a unique

A

Atomic Emission Spectrum

30
Q

Wavelength of light emitted from a star can be used to determine what elements it comprises by resolving the star’s component

A

Wavelengths

31
Q

The group of hydrogen emission lines corresponding to transitions from n>2 to n=2 is known as the

A

Balmer Series

32
Q

The group of hydrogen emission lines corresponding to transitions between upper levels n>1 to n=1 is known as the

(higher energy transitions that occur in the UV region)

A

Lyman Series

33
Q

The energy associated with a change in the euantum number from an initial value to a final value is equal to the energy of Planck’s emitted photon. What is the equation that represents this?

A

E=hc/λ = -R(H)(1/ni^2 - 1/nf^2)

34
Q

In addition to an emission spectrum, this is formed when an electron is excited to a higher energy level and is characteristic of each element.

A

Absorption Spectrum

35
Q

Are the wavelengths of the absorption and emission spectrum the same?

A

Yes.

36
Q

Bohr’s model offered a reasonable explanation for the structure of the hydrogen atom but does not explain structures of atoms containing more than 1 electron. Why?

A

Bohr’s model does not take repulsion between multiple electrons surrounding one nucleus into account

37
Q

State the Heisenberg uncertainty principle

A

It is impossible to determine with perfect accuracy both the momentum and position of an electron simultaneously.

If one is measured,the other will change, and vice versa

38
Q

Bohr’s model also incorrectly assumed that electrons move in circular orbits. What is correct?

A

Electrons move in orbitals

39
Q

This states that no two electrons in a given atom can possess the same set of four quantum numbers.

A

Pauli Exclusion Principle

40
Q

The position and energy of an electron is described by quantum numbers, also called its

A

Energy state

41
Q

The principal quantum number is letter…
The angular momentum quantum number is letter…
The magnetic quantum number is letter…
The spin quantum number is letter…

A

n
l
ml
ms

42
Q

The maximum number of electrons in an energy level n is…

A

2n^2

43
Q

The energy difference between the third and fourth shells is more or less than that between the second and third shells?

A

Less

44
Q

For any given n, the value of l can be any integer in the range of..

l refers to the ____ that occur within each principal energy level

A

0 to n-1

subshells/sublevels

45
Q

The maximum number of electrons that can exist in a subshell/sublevel

A

4l+2

46
Q

Greater l means greater energy,. However, energies of subshells from different principal energy levels may overlap. For example, 4s will have a higher/lower energy than the 3d subshell

A

lower.

The average distance of 4s from the nucleus is smaller than 3d

47
Q

l=0,1,2,3

A

s,p,d,f subshells

48
Q

This quantum number designates the particular orbital within a subshell where an electron is highly likely to be found at a given point in time. This orbital can contain no more than 2 electrons

A

magnetic quantum number (ml)

49
Q

The possible values of ml are…

A

-l to +l

50
Q

The three dumbell shaped orbitals that are oriented around the nucleus are referred to as..

A

px,py,pz

51
Q

This quantum number that is the particle’s intrinsic angular momentum.

A

spin quantum number (ms)

52
Q

Electrons in the same orbital must have ____ spins

Electrons in different orbitals with the same ms values are said to have ____ spins

A

Opposite

Parallel

53
Q

When writing the electron configuration of an atom, it is necessary to remember the order in which subshells are filled. Subshells are filled from lowest/highest energy to lowest/highest energy

A

Subshells are filled from lowest energy to highest energy

54
Q

Hand’s Rule states that within a given subshell, orbitals are filled such that there are a maximum number of half-filled orbitals with OPPOSITE/PARALLEL spins?

A

Hand’s Rule states that within a given subshell, orbitals are filled such that there are a maximum number of half-filled orbitals with PARALLEL spins

55
Q

According to the book, subshells may be listed in the order in which they fill or with subshells of the same principle quantum number grouped together. Either is correct.

A

Mmkay.

56
Q

A material with unpaired electrons that is weakly attracted to magnetic fields because of realignment is called

A material with paired electrons that is not attracted to magnetic fields is called

A

Paramagnetic

Diamagnetic

57
Q

If all molecules in a given problem have the appropriate number of protons and neutrons, what else determines their radioactivity?

A

If they have odd numbers of protons and neutrons

DAT GenChem (11 decks)

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