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Intro to basic chem Flashcards

1
Q

What is the atomic number of an atom

A

Number of protons in the nucleus ***determines what element it is

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2
Q

What is the mass number of an atom

A

Number of protons + neutrons

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3
Q

What is an isotope

A

Same element but with a different number of neutrons

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4
Q

Describe what metals often do in terms of charge and bonds

A

Tend to lose elections to form positive ions to obtain Noble gas configuration
Then can form ionic bonds with negative ions that are usually non metals

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5
Q

What are the 4 characteristics of metals that are explained by the electron sea model which states an array of metal nuclei exists in a sea of valance electrons

A

Ductile (stretchable)
Malleable (hammer into strips)
Conductive (electric and thermal)
Luster (shinny)

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6
Q

Describe characteristics of non metals and their type of bonding

A

Tend to form negative ions
Bind covalently with other non metals and ionic bonds with positive ions
Poor conductors, non malleable, brittle, and low melting points

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7
Q

What is effective nuclear charge (Zeff)

A

Net positive charge from the nucleus felt by an orbiting electron

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8
Q

Trend of effective nuclear charge on the periodic table

A

Increases going left to right and top to bottom

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9
Q

Trend of atomic radium on the periodic table

A

Increases from right to left and top to bottom

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10
Q

What is ionization energy and the trend on the periodic table

A

Energy required to remove an electron from a neutral gaseous atom
Increases from left to right and bottom to top

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11
Q

How does gaining or losing electrons change the size of ions

A

Cations are smaller bc less electrons

Anions are larger bc more electrons

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12
Q

What is electronegativity and its trend on their periodic table

A

Ability of an atom to attract the shared electrons in a covalent bond (electrons to itself)
Increases left to right and bottom to top
***fluorine most electronegative

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13
Q

What is electron affinity and its trend on the periodic table

A

Energy change when an atom gains an electron

Increases from left to right and bottom to top

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14
Q

Explain what it means that noble gasses have positive electron affinity values

A

It would take energy to add an electron bc they are stable as is
EA values are always positive bc adding the electron is endothermic

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15
Q

Why is the first EA negative and the second positive

A

Energy is released in the first addition of the electron bc it is attracted to the positive Zeff
For the second EA onwards energy is needed to overcome electrostatic repulsion of adding another electron to a negative ion

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16
Q

What do they mean by quantum mechanics

A

Electrons can only gain or lose energy in discrete quantities

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17
Q

What is the principal quantum number

A

Energy level and average distance from the nucleus

N = 1,2,3…

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18
Q

What is the angular momentum quantum number

A 
Orbital shape 
0 to n-1
L = 0 = s
L = 1 = p
L = 2 = d
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19
Q

What is the magnetic quantum number

A

Orbital orientation
- l to +l
If l = 0 there is only one orientation but for l = 1 there are orientations along x,y,and z

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20
Q

What is the spin quantum number

A

Either 1/2 or - 1/2

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21
Q

Electrons are not at a single point what is an atomic orbital

A

Areas of space where you are likely to find an electron

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22
Q

What are the orbital shapes

A

S - sphere
P - dumbbell (3)
D = clover leaf except one bow tie (5)

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23
Q

What is the aufbau principle

A

Electrons will always occupy lowest energy spot when multiple electrons are present

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24
Q

What is hunds rule

A

Electrons will fill each sub shell before base pairing

25
What is the Pauli exclusion principle
No two electrons in an atom can occupy the same space therefore no two electrons can have the same 4 quantum numbers
26
What does isoelectronic mean
When atoms and ions have the same electron configuration | Br- = Kr
27
Can you add energy to move an electron into a higher level
Yes if it is the correct amount
28
Half filled and filled shells are extremely stable, give some examples of transition metals that promote electrons from nearby orbitals
``` Chromium Copper Silver *** take a look at what the electron configuration would be **** groups 1,2, 7,12,15, and 18 ```
29
What is the difference between diamagnetic and paramagnetic electrons
Para - unpaired electrons which have a magnetic field | Dia - spin paired electrons so magnetic field cancels out
30
What happens if you change the number of neutrons, electrons or protons respectively
Isotope Ion New element
31
Properties of alkali metals
Easily form +1 cations Highly reactive with non metals to form ionic compounds *hydrogen is not the same
32
Properties of alkaline earth metals
Harder more dense with a higher melting point than alkali Form 2+ cations Exist only as compounds in nature but are less reactive
33
Describe group 14 elements
Can form four covalent bonds with nonmetals | Only carbon can make pie bonds
34
Describe group 15 elements
Can form 3 covalent bonds Nitrogen can donate its lone pair of electrons to form a bond Nitrogen can form strong pie bonds
35
Describe oxygen bonding abilities
Can form strong pie bonds to make double bonds Second most electronegative element Reacts with metals to form metal oxides
36
Describe sulfur bonding abilities
Can form many more bond than oxygen due to 3D orbital | Can form pie bonds
37
Describe group 17 elements
Highly reactive like to gain an electron
38
Describe group 18 elements
Noble gases that are non reactive | Tend to exist as diatomic molecules
39
Describe the equation KE = hf - work function
Hf is the energy put in by a photon and then the work function is the min amount of energy required to eject an electron The electron is only emitted if the photo has enough energy Kinetic energy is the excess energy from the photon and determines the speed the electron moves away from the metal
40
Describe electromagnetic radiation energy
As energy travels forward electric and magnetic fields are created perpendicular to each other and to the direction of travel
41
What is the frequency of a wave
Number of crests or troughs that pass through a giver point per second Wavelength/velocity —- hertz
42
Name the wavelengths in increasing frequency
``` Tv/radio waves Microwaves Infrared Visible Violet X-ray Gamma ```
43
What is the relationship between mass and wavelength according to de broglies postulate
Inversely proportional
44
Describe ionic bonds
Metal and non metal Complete transfer of ions forms cation and anion Stronger than covalent
45
Describe covalent bond
Share electrons , similar electronegativity | 2 non metals
46
What happens when two atoms form a covalent bond where the electrons aren’t shared equally
Polar covalent bond that contains a dipole where the arrowhead points to the electron rich region **** has a direction so it is a vector
47
What are pure covalent bonds
Non polar occur between identical atoms | No difference in electronegativity so the electrons are shared
48
Non polar molecules with polar covalent bonds to watch out for on the MCAT
Symmetric with no net dipole moment as they can each other out CO2 CCl4 BF3
49
Difference between inter and intra molecular binding
Inter - weak interactions between molecules | Intra - sharing electrons with same molecule ***much stronger
50
3 types of intermolecular forces (van der waals) from weakest to strongest
1. London dispersion - shifting of electron cloud to make induced dipoles 2. Dipole - dipole 3. Hydrogen bonding - H with O F or N - stronger than the others makes higher boiling/melting point (H2O) but still not near as strong as intramolecular forces
51
What is radioactive decay
Unstable nuclei are radioactive as the number of protons or neutrons change it becomes more stable over time
52
What is alpha decay
Emits an alpha particle containing 2 protons and 2 neutrons Mass -4 Atomic # - 2
53
What is negative beta decay
Neutron breaks down into a proton and electron , the electron (beta ) is emitted +1 atomic #
54
What is positive beta decay
Proton turns into a neutron , positron is emitted | -1 atomic #
55
What is electron capture
When nucleus has too few neutrons a core electron is captured and combined with a proton to form a neutron -1 atomic #
56
What is gamma decay
When excited nucleus relaxes gamma rays are emitted so basically useless doesnt change anything
57
What is the Heisenberg principle
The momentum and position of an electron cant be known with certainty at a time
58
Electron configuration of a metal atom vs ion
Atom would be what you expect but if they ask for the ion form then generally the metal will loss electrons to get a positive charge and have a similar configuration to the noble gas
59
Electron configuration of non metal atom vs ion
Non metals will gain electrons to have the same configuration as the nearest noble gas which is the configuration you use if they ask for the ion

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