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Uworld > Gen Chemistry > Flashcards

Gen Chemistry Flashcards

1
Q

Alpha decay is

A

Two protons and two neutrons (-4 from up and -2 down - atomic number

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2
Q

Beta decay is

A

+1 electron

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3
Q

Electron capture is

A

-1 electron (beta plus decay)

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4
Q

Only … tend to lose or gain as many electrons as needed to achieve a full octet

A

Neutral atoms

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5
Q

Definition of effective nuclear charge

A

Measure of the amount of charge from the nucleus of an atom or ion that exerts electrostatic attraction on its valence electrons

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6
Q

Formula of Zeff

A

Zeff= Z (total charge= total number of protons) - S (core electrons =10)

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7
Q

Electron configuration order

A

1s 2s 2p 3s 3p 4s 3d 4p 5s

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8
Q

Types of beta decay

A

B- decay is electron emission, B+ is positron emission and electron capture (decreases atomic number, proton to a neutron) while the mass number is the same

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9
Q

Volume formula

A

Mass/volume

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10
Q

As temperature decreased the density of the solution … and objects .. while when the t increases..

A

Increases, floats

Density decreases and object sinks

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11
Q

1 mole is how many units and g ?

A

6* 10^23 units and mass of the molecule in g

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12
Q

Name of the reaction when both the oxidation and reduction occurs to atoms of the same element

A

Disproportionation reaction

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13
Q

Slope

A

(y2-y1) / ( x2 -x1)

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14
Q

What agent get oxidized and causes reduction in another atom

A

Reducing agent

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15
Q

What agent that gets reduced and causes oxidation in another atom?

A

Oxidizing

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16
Q

Formal charge formula

A

Valence electrons - no binding electrons- 0.5 bonding electrons

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17
Q

Oxidation state formula

A

Group valence - non bonding electrons - assigned bonding electrons ( electrons are given to the most electronegative atom of the bond)

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18
Q

Molarity formula

A

Mol / volume

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19
Q

Principal quantum number is

A

n shell describes main energy level of the electron
Distance of an orbital from the nucleus

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20
Q

Sub shell is

A

Shape of an orbital s, p, d, f and holds 2,6,10,14 electrons

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21
Q

Diamagnetic means

A

All electrons are paired and repelled by external magnetic field

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22
Q

Paramagnetic means

A

Unpaired electrons that pulled into external magnetic field

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23
Q

Gamma emission means

A

Change in energy, mass number and atomic number are not changed

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24
Q

As IE increases the Reactivity of atoms …

A

Decreases and vice versa

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25
Q

Definition of electronegativity

A

Tendency of an atom to attract electrons within a bond

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26
Q

Definition of electron affinity

A

Tendency of an atom to accept an additional electron by measuring the energy change when an electron is added

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27
Q

Definition of ionization energy

A

Measures energy required to remove an electron from the atom (opposite of affinity)

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28
Q

Definition of a polarizability

A

Extent to which an electron cloud of an atom can be distorted by an external charge or by an applied electric field to produce a dipole

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29
Q

First IE definition

A

Removal of the first electron

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30
Q

Second IE definition.

A

Removal of the second electron

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31
Q

What takes more energy to remove an electron: valence electron or core electron?

A

Core electron ( metal have lower IE energy than nonmetals)

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32
Q

STP numbers are

A

0 C or 273 K
1 atm
1 mol of gas = 22.4 L

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33
Q

Positron emission is what type of decay?

A

Beta + decay

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34
Q

When the atoms are more stable?

A

When they have a full outer orbital shell

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35
Q

What properties share elements in the same column?

A

Just chemical (valence configuration)!!
Not physical (diff number of neutrons)!!

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36
Q

Nuclear fission definition

A

Splitting of a large atomic nucleus into multiple smaller nuclei

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37
Q

Isotope definition

A

Atoms share the same atomic number but different mass number( neutrons, density), same chemical properties but not physical

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38
Q

No polar means

A

EN less than 0.5

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39
Q

Polar means

A

EN from 0.5 to 1.7

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40
Q

Ionic bond means

A

Nonmetal plus metal, attraction of opposite charges.
Differences in electronegativity greater than 1.7

41
Q

Covalent bond means

A

Electrons are shared between atoms

42
Q

More electronegative atoms means that it has

A

Stronger attraction, valence electrons closer to the nucleus and less core electrons

43
Q

As bond order increases then its bond strength

A

Increases, bond energy increases but bond length decreases

44
Q

Relationship between atomic radii and bond length

A

More atomic radii has more bond length

45
Q

As IE decreases the number of core electrons … which results

A

Increases and the noble gas is more stable as less attraction to the nucleus

46
Q

As the size of an atom increases the polarizability …

A

Increases as well

47
Q

Energy of a photon is directly proportional to … but inversely to …

A

its frequency
To its wavelength

48
Q

Bohr model

A

Farther orbits = higher energy = shortest wavelength
Photon emitted when n decreases and absorbed when n increases

49
Q

Empirical formula means

A

Ratio of each type of atom
By moles

50
Q

Molecular formula means

A

Actual number of each type of atom

51
Q

Structural formula means

A

How the atoms are bobsled to one another

52
Q

In isoelecteonic atoms ionic radii decreases when

A

Atomic number increases

53
Q

Size of anions and cations

A

Anions are bigger than cations

54
Q

Combustion reaction definition

A
55
Q

What diatomic atom makes a single bond?

A

H2, F2, Cl2, Br2, I2

56
Q

What diatomic atom makes a double bond?

A

O2

57
Q

What diatomic atom makes triple bond?

A

N2

58
Q

Electrical conductivity tendency

A

Metals are the most vindictive then metalloids and then no metals( least conductive)

59
Q

Valence shell diagram

A
60
Q

Higher IO then reactivity is

A

Lower

61
Q

Representative elements on the table are

A

s and p block ( groups 1-2, 13-18)

62
Q

Reactivity of alkaline metals increases when

A

Atomic number increases

63
Q

Oxidation definition

A

Reducing agent gives up electrons ( increases at the product)

64
Q

Reduction definition

A

Oxidizing agent takes electron (decrease in products)

65
Q

Concentration ratio

A

Stock solution/ standard solution

66
Q

Dilution factor

A

Volume of the diluted solution/ volume of original solution

67
Q

What happens during gamma emission?

A

Unstable nucleus in an excited state released excess energy by emitting a gamma ray which is a high energy photon without ejecting a particle

68
Q

Orbital angular momentum quantum number

A

l (sub shell type: s, p, d or f)
Describes shape of the orbital where l = 0,1,2,3… (n-1)

69
Q

Magnetic quantum numbers

A

ml determines number of orbitals and their orientation
All ranges from -l to +l

70
Q

Electron spin quantum number

A

Ms angular momentum of an electron 1/2 spin up or down

71
Q

Adding an electron is easier for what group?

A

Nonmetals

72
Q

Why are noble gases the least reactive group?

A

They have a full valence shell configuration (full s and p except for He-only full s)

73
Q

Reactivity of the atom means

A

Tendency to gain, lose or share electrons

74
Q

Smaller atomic radius makes a bond

A

Stronger and smaller
Making it a weak acid

75
Q

Large atomic radius makes bond to be

A

Longer and more acidic

76
Q

Small electron affinity means

A

Increases electron electron repulsion between valence electrons

77
Q

The most electronegative atom has an increased electron density creating a

A

Dipole

78
Q

Lewis base is .. while Lewis acid is..

A

An electron donor,
Electron acceptor

79
Q

Arrhenius base is a … while an acid is..

A

OH- donor, H+ donor

80
Q

Brønsted-Lowry acid is a … while a base is a..

A

H+ donor, H+ acceptor

81
Q

Metals ions in coordination chemistry act as

A

Lewis acids

82
Q

Lewis based in coordination chemistry are

A

Ligands that coordinate with the metal ion

83
Q

Heisenberg uncertainty principle definition

A

Exact position and momentum can’t be known both at the same time, just one of them where electrons in coordination bonds can be described only as probability distributions

84
Q

Pauli exclusion principle

A

Two electrons in the same orbital must have opposite alignment

85
Q

Types of magnetism

A
86
Q

Control group is one that

A

Absent of independent variables

87
Q

Contrast agent definition

A

Increase mri signals by increasing the relativity of water molecules to monitor biological processes

88
Q

Atom can absorb a single photon with an energy equal ..

A

To the energy difference between the two states

89
Q

Third IE is higher than the second IE because

A

It needs to remove a core electrons meaning it requires more energy to remove the electron as it tightly held

90
Q

S orbital electrons requires more energy than p orbital because

A

It holds tightly therefore requires more energy to remove the electron

91
Q

Dipole characteristics and types

A

Consists of opposite electric charges separated across a distance. In molecules, permanent dipoles form across some covalent bonds due to unequal sharing of electrons between two atoms caused by large differences in electronegativity. In a dipole, region with greater electron density gains (higher electronegativity between atoms) a partial negative charge while with less electron density ( higher electronegativity) positive charge.
Types: dipole-dipole - when the opposite charges of the polar bonds form a mutual attraction. Ion - dipole interaction - full charge of ion attracts the opposite charge of a polar bond dipole.
Dipole induced interaction - dipole form the polar bond distorts the electron cloud of a nonpolar bond and induced a weak attraction. London forces - form when two nonpolar bonds induce momentary dipole.

92
Q

Electrolytes and compounds conductivity characteristics

A

Electrolyte - are solute that enable the conduction of electricity within a solvent (like NaCl).
Ionic compounds (metal + nonmetal) are conductive in liquid form but not in solid.
Metallic compounds - conductive in both solid and liquid states and have a high MP.
Molecular compounds - covalently bonded nonmetals and not conductive in both states.

93
Q

Balanced net ionic equations conserve both …

A

Number of atoms and the net charge

94
Q

Theoretical yield definition

A

Maximum amount of product that can form if all the limiting reactant is converted into products.
The amount of product that can be isolated from a fraction cannot exceed the theoretical yield.
The actual yield is always less than the theoretical because no reaction is perfect due to loss.

95
Q

Double replacement reactions

A

Two compounds form two new compounds (ion swap)

96
Q

Single replacement reaction

A

With a free element.

97
Q

Ligand exchange via a … but their … are unchanged

A

Coordinate bond, oxidation numbers

98
Q

Methods to test proposed mechanisms are

A

Certifying the reactions rate law,
Detecting an intermediate, interfering with a mechanistic pathway.

Having the same leaving groups is not a method !!!

99
Q

Dipole moment is

A

u = qr where q- magnitude of the partial charge (increased when the the difference in electronegativity between two atoms increased and vice versa) and r - distance

Uworld (24 decks)

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