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Chapter Seven
Atomic Structure and Periodicity - Wavelengths, shells, atoms
28
Chemistry
Undergraduate 1
11/15/2011

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Term
Convert hertz to megahertz
Definition

1 Hz = 1.0 × 10-6 MHz


1 MHz = 1.0 x 106 Hz 

Term
Planck's Constant (h)
Definition
6.626 x 10-34 J.s
Term
Speed of light (c)
Definition
2.99 x 108 m/s
Term
Energy of a photon
Definition

Ephoton = hv = hc

                    λ

 

Term
Dual nature of light
Definition
Light can be emitted as a wave as well as particles.
Term
Electron Configuration
Definition
1s2s22p63s23p4s23d104p5s24d105p6s24f145d106p7s25f146d107p6
Term

Ionization Energy 

When does it increase/decrease and why?

Definition

*IN GAS PHASE*

 

- Increases (harder to remove e-) from left to right.

This is because there the electrons are more tightly bound as you go from left to right and it is harder to remove.

- Decreases (easier to remove e-)from up to down.

This is because the electrons being removed are farther from the nucleus and therefore, the electron is easier to remove.

 

Term

Electron Affinity 

When does it increase/decrease and why?

Definition

*IN GAS PHASE*

 

- Generally, increases (more negative - more E is released) from left to right because as you go through a period, the elements become more willing to gain electrons.

- Generally, decreases (becomes more positive - less E is released) from up to down because the orbitals are increasing in size and the electron is added further away from the nucleus.

Term

Electron Affinity

What is it?

Definition

The energy change associated with the addition of an electron to a gasous atom:

 

X(g) + e- --->X-

Term

Ionization Energy

What is it?

Definition

Energy required to remove an electron from an atom

 

X --> X+ + e-

Term

Atomic Radius

When does it increase/decrease and why?

Definition

- Decreases from left to right.

This is because the valence electrons are drawn closer to the nucleus, decreasing the size of the atom.

- Increases from up to down.

This is because of the increase in orbital size.

Term
Hund's Rule
Definition

Lowest electron configuration for an atom is the one having the maximum number of unpaired electrons allowed by pauli principle in a particular set of degenerate orbitals.

 

2P ^  ^  ^ lower than 2P ^v  ^

Term
DeBrogile's Wavelength Equation
Definition
wavelength = h/mv
Term

What makes X3+ smaller than X2+

ex) Al3+ < Al2+ < Al+ < Al

Definition
Because when the nucleus is more positive, the electrons are drawn closer to the nucleus and it's smaller.
Term
Why would the ion X4+ have a higher electron affinity than X3+?
Definition
Because the X4+ has the most exothermic electron affinity; it releases the most energy when adding an electron.
Term
Why would there be such a large jump in removing electrons from an ion?
Definition
Because once you start removing electrons that are close to the nucleus, it requires more energy. If you remove all the valence electrons and try to remove a core electron, it will be very difficult and require a lot more energy.
Term
Breaks in Trends 
Definition

Ionization Energy – Between nitrogen and oxygen, there is a break in the trend because oxygen is more willing to lose its electron due to electron repulsion.

Electron Affinity – Between carbon and nitrogen, there is a break in the trend because nitrogen is more unwilling to gain an electron due to electron repulsion.

Term
Principle Quantum Number
Definition

n - whole numbers from 1, 2, 3,...

 

Refers to size of orbital

Term
Angular Momentum Number
Definition

L - 0, 1, 2,...(n-1)

 

Refers to shape of orbital

 

L=0, S (sphere)

L=1, P (figure eight)

L=2, D (flowerything)

L=3, F

Term
Magnetic Quantum Number
Definition

mL : -L...0...L

Orientation of orbital

1 = s = 1 orbital = 2 electrons

2 = p = 3 orbitals = 6 electrons

3 = d = 5 orbitals = 10 electrons

4 = f = 7 orbitals = 14 electrons

Term
Convert nanometers to meters
Definition
1 nm = 10-9 m
Term
Wavelength/Frequency Formula
Definition

Frequency:       ν = c/λ


Wavelength:     λ = c/ν

Term
Bohr’s Model
Definition

A hydrogen atom’s e- moves around the nucleus only in certain allowed circular orbits. This was proved false for anything other than the H atom.

Term
Aufbau Principle
Definition

As protons are added one by one to the nucleus to build up the elements, electrons are added to these hydrogen-like orbitals (square method)

Term
Degenerate Orbitals
Definition

 

All orbitals with the same value of n have the same energy.

Term
ψ – wave function
Definition

 the coordinates of an electron’s position in three-dimensional space. A specific wave function is called an orbital. Developed by Schrodinger.

Term
Energy Level of H atom
Definition

 E = –2.178 x10-18 (z2/n2),

 

where n is the level, z is the atomic number

Term
Electron Spin
Definition
2 Ml =Ms = number of electrons in that shell – there can only be two values: -½ and +½
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