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Chemisty Honors > Unit 2: Quantum and Periodic Table > Flashcards

Unit 2: Quantum and Periodic Table Flashcards

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1
Q

Quantum

A

How matter and energy interact

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2
Q

Niels Bohr

A

Used the research and discovery of pervious scientists to come up with a system consisting of a small, dense nuclear surrounded by orbiting electrons

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3
Q

Bohr’s Planetary Model of the Atom

A

Electrons travel in definite energy levels without radiating energy, electrons in each orbit have a certain amount of energy, energy increase as distance from the nucleus increases, electrons will lose energy

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3
Q

Planetary Model (Bohr Model)

A

Electrons can gain energy when heated, electrons gain this energy in small specific amounts called quanta, electrons are said to be excited after it gains a quanta of energy

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4
Q

Quanta

A

The small specific amounts of energy gained by electrons

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5
Q

Ground State

A

The lowest energy state of an atom

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6
Q

Excited State

A

A state in which an atom has a highest potential energy than it has in its ground state

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7
Q

Quantum

A

The minimum quantity of energy that can be lost or gained by an atom

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8
Q

Photon

A

A particle of electromagnetic radiation having zero rest mass and carrying a quantum of energy

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8
Q

Emissions Spectrum

A

The range of wavelengths emitted by an atom or compound stimulated by either heat or electric current (excited state)

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9
Q

Absorption Spectrum

A

The range of wavelengths absorbed by an atom or compound (the sample is not stimulated) (ground state)

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10
Q

Atomic Emissions Spectrum

A

The set of frequencies of the electromagnetic spectrum emitted by the excited electrons of an atom, will produce only a few lines of specific colored light, produced by hot gases giving off energy in the form of photons

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11
Q

Inadequacy of the Bohr Model

A

The bohr model explained the energy absorbed and emitted by the hydrogen atom which contains one electron; but it failed to explain more complex atoms

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12
Q

Quantum Theory

A

Describes mathematically the wave properties of electrons and other very small particles, was proposed by Max Planck

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13
Q

Planck’s Constant

A

States that atoms can only gain or lose electrons in certain amounts, this is the least amount of energy that can gained or lost by an atom, there is no inbetween, energy gain or loss is incremental, planck’s constant is 6.626x10^-34 J

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13
Q

Electromagnetic Radiation

A

A form of energy that exhibits wavelike behavior as it travels through space, all the forms of electromagnetic radiation come together to form the electromagnetic spectrum

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14
Q

Velocity

A

The speed in a given direction

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15
Q

Wavelength

A

The distance between two waves

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16
Q

Frequency

A

The number of waves during a period of time

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17
Q

Amplitude

A

The height of a wave

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18
Q

Speed of light

A

c= 3.00x10^8 m/s

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19
Q

Wave properties of electromagnetic radiation

A

Waves with low energy have low frequency and a big wavelength, waves with high energy have a high frequency and a small wavelength

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19
Q

Wavelength and Frequency (relationship)

A

inverse relationship

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20
Q

Energy and Frequency (relationship)

A

direct relationship

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20
Wavelength and Energy (relationship)
Inverse relationship
21
Photoelectric Effect
A phenomenon where electrons are emitted from the metal surface when the light of sufficient frequency is found, Albert Einstein suggested this idea, used planck's idea that a light is a particle (photon)
22
De Broglie's Hypothesis
All matter exhibits wave-like properties and relates the observed wavelength of matter to its momentum, so the wave particle duality
23
Wave Particle Duality
The concept in which quantum entities exhibit particle or wave properties according to experimental circumstances
24
Heisenberg Uncertainty Principle
It is impossible to determine both the position and velocity of an electron or any other particle at the same instance, helped to develop the modern quantum theory, we cannot be certain where electrons are at any given moment
25
Schrodinger's Wave Equation
Predicts analytically and precisely the probability of events or outcome of a wave based on the energy and momentum of an electron
26
Quantum Model
The quantum mechanical model of the atom uses complex shapes of orbitals (sometimes called electron clouds), volumes of space in which there is likely to be an electron, this model is based on probability rather than certainty
27
Orbitals
A 3d region around the nucleus that indicates the probable location of an electron
28
Aufbau Principle
An electron occupies the lowest-energy orbital that can receive it
29
Hund's Rule
Every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons is singly occupied have the same spin
30
Pauli Exclusion Principle
No two electrons in the same atom can occupy the same space, no two electrons can be at the same place at the same time
31
Lewis e- Dot Diagrams
Shows the number of valence electrons for an atom
31
Valence Electrons
The outermost electrons of the atom
32
Cation (ion)
Lost valence electron (e-)
32
Antion (ion)
gain valence electron (e-)
33
Demtri Mendeleev
Designed the first periodic table of elements, arranged elements by increasing atomic mass, predicted properties of missing elements and left empty spaces for them
34
John Newland
First person to devise a periodic table of elements arranged in order of their relative atomic weights
34
Henry Moseley
Arranged the periodic table by atomic number, created the modern periodic table
34
Modern Periodic Table Law
States that the physical and chemical properties of the elements are the periodic functions of their atomic numbers, scientists arranged elements in increasing order of their atomic number from left to right across each row
34
Metals (10 things)
Malleable, Ductile, good conductors, lustrous (shiny), low ionization energy, low electronegativities, loses electrons easily, high melting points and boiling points, few valence electrons
35
Non-metals (10 things)
Brittle solids, dull, high ionization energy, high electronegativites, gains electrons easily, poor conductors, usually liquids or gasses at room temperature, low melting and boiling points, 5-8 valence electrons
35
Metalloids (4 things)
Lustrous (shiny), brittle, fair conductors (semi-conductors), acts like non-metals when bonding
35
Periodic Table Groups (group names)
Alkali Metals, Alkaline Earth metals, Transition metals, Metalloid, Halogens, Noble Gases, Lanthanides, Actinides
35
Periodic Table Groups (definition)
Element in the same group have similar characteristics, elements in the same group have the same number of valence electrons, elements in the same group make similar bonds
35
Periods of the periodic table
All the elements in a period have the same number of atomic orbitals within the same energy level, elements in the same row have something in common with one another
35
Alkali Metals
group 1, soft, most reactive metals, one valence electron, reacts violently with water, not found in pure form in nature
35
Alkaline Earth Metals
group 2, are very reactive, more dense than group 1, harder than group 1, less reactive than group 1, two valence electrons, not found in pure form in nature (used in fireworks, batteries, and your body)
35
Transition Metals
D block, metallic properties =, forms colored ions in solution (think of copper), more than one charge (ions like copper can be +1 or +2), most widely used by humans (less reactive, harder, and stronger than groups 1&2)
35
Inner Transition Metals
F block, Lanthanides and Actinides, often used with light and film, uranium is in this section (nuclear power)
36
Lanthanides
Rare earth metals, similar to group 2 in characteristics, top row of F block
36
Actinides
Radioactive, bottom row of F block
37
Metalloids
Staircase (except Aluminum), exhibits characteristics from both metals and nonmetals, semiconductors,
38
Halogens
Group 17, most reactive nonmetals, called salt formers, 7 valence electrons
38
Noble Gases
Group 18, all of these elements are gases, they don't interact with other elements
39
Other groups
named by elemet at the top of the table, some groups are mixed with metals and nonmetals
40
Atomic Radius
The distance from the center of the nucleus to the outer valence shell or half the distance of a bond
41
Atomic Radius (across a row)
Decreases due to increasing coulombic attraction, e- held more tightly (more p+ in the nucleus)
41
Atomic Radius (down a group)
Increases due to decreasing coulombic attraction because added more energy levels
41
Coulombic Attractions
The increasing difference between the positive charge of the nucleus and the negative charge of the electrons, this causes the electrons to be held more tightly to the nucleus
42
Ionic Radius
Cation: decreases atomic radius Na > Na^+1, Anion: increases atomic radius Cl > Cl^-1
43
Reactivity
Determined by how willing an atom is to form a new bond, the more reactive the more likely a new bond will form
44
Metal Reactivity
Increases as you move to the left and down the periodic table (francium is the highest)
45
Nonmetal Reactivity
Increases as you move to the right and up the periodic table (florine is the highest)
46
Ionization energy
The amount of energy needed to remove an outermost e-
46
Ionization energy (across a row)
Increases due to increasing number of p+, increasing coulombic attraction, greater pull on e-, harder to remove =, requires more energy
47
Ionization energy (down a group)
Decreases due to decreasing coulombic attraction because increasing number for energy levels, e- is farther from the nucleus, easier to remove, requires less energy, increased shielding by inner e- will also decrease the energy required
48
Electron affinity
Attraction a non-bonded atom has for an additional; e- (so is a measure of the attraction between the incoming electron and the nucleus)
49
Electronegativity
Ability for a nucleus to attract a e-, fluorine has the highest electronegativity, the noble gases have an electronegativity of zero
50
Factors that can affect periodic table trends (Nuclear charge)
coulombic attraction, affects pull on e- cloud
51
Factors that can affect the periodic table trends (atomic size)
number of energy levels affects the distance between the nucleus and valence e-
52
Factors that can affect periodic table trends (shielding)
Number of e- between the nucleus and valence e-
53
Factors that can affect periodic table trends (sublevel stability)
1/2 and full sublevels are more stable than other configurations

Chemisty Honors (3 decks)

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