Chapter 3 Flashcards
Speed of Light (c)
2.998x10^8 m/s
Wavelength (λ)
distance between two consecutive peaks or troughs in a wave
Frequency (v)
number of successive wavelengths that pass a given point in a unit of time
Amplitude
one-half the distance between the peaks and troughs
Unit for Frequency
hertz (Hz)
MHz –> Hz
1 –> 10^6
GHz –> Hz
1 –> 10^9
Speed of the Wave
λv
As the wavelength increases, the frequency…
decreases
As the frequency increases, the wavelength…
decreases
Planck’s Number (h)
6.626x10^-34 Js
E=
hv
v=
c/λ
Ground State (of an atom)
occurs when the electron is in the lowest energy orbit (n=1)
Excited State (of an atom)
occurs when it is possible for the electron to move to an orbit with a higher n-value, which has higher energy
An atom absorbs energy and the electron moves…
from a lower n to a higher n
An atom emits energy and the electron moves…
from a lower n to a higher n
Energy of Electron Orbital Movement (equation)
ΔE=k{[1/(n1)^2]-[1/(n2)^2]}
k=
2.179x10^-18 J
Principal Quantum Number or Shell Number
n
Angular Momentum Quantum Number
l
For l=0
s orbital
For l=1
p orbital
For l=2
d orbital
For l=3
f orbital
of Possible S Orbital Shapes
1
of Possible P Orbital Shapes
3
of Possible D Orbital Shapes
5
of Possible F Orbital Shapes
7
Magnetic Quantum Number
m
Spin Quantum Number
ms
ms=
1/2 or -1/2
Pauli Exclusion Principle
no two electrons in the same atom can have exactly the same set of all four quantum numbers
Subshell Electron Capacity (low —> high E)
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p
Aufbau Principle
Add the number of electrons equal to the atomic number one at a time to the subshell of the lowest available energy
Core Electrons
electrons occupying the inner shell orbitals
Valence Electrons
electrons occupying the orbital(s) in the outermost shell (highest value of n)
Electron Configuration of Cu
[Ar] 4s1 3d10
Electron Configuration of Cr
[Ar] 4s1 3d5
Periodic Trend (size or radius)
increase down a group and decreases across a period
A cation is always ___ than the atom from which it is derived
smaller
A anion is always ___ than the atom from which it is derived
larger
Isoelectronic
atoms and ions that have the same electron configuration
Periodic Trend (ionization energy)
amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state
decreases down a group, increases across a period
Be (4) has a ___ IE than B (5)
higher
O (8) has a ___ IE than N (7)
lower
removing an electron from a CATION is ___ than removing an electron from a neutral atom
harder
Electron Affinity (EA)
the energy change for the process of adding an electron to a gaseous atom to form an ANION
A negative EA means…
energy is released (exothermic)
A positive EA means…
energy is required (endothermic)
Periodic Trends (electron affinities)
more negative EA across a period
Deviations to EA Trend
group 18 (filled shell), group 2 (filled ns subshell), group 15 (half-filled np subshell)
Metals (left)
shiny, malleable, good conductors of heat and electricity
Nonmetals (right)
appear dull, poor conductors of heat and electricity
Metalloids (touching staircase - Al)
conduct heat and electricity moderately well, possess some properties of metals and some properties of nonmetals
Group 1 (except hydrogen)
alkali metals
Group 2
alkaline earth metals
Group 17
halogens
Group 18
noble or inert gases
Ionic Bonds
electrostatic forces of attraction caused by the transferring of electrons
- metals form cations
- nonmetals create anions
Covalent Bonds
caused when electrons are shared between two nonmetals
Properties of Ionic Compounds
- solids typically have higher melting and boiling points
- nonconductive in solid form
- conductive in molten form
Properties of Covalent Bonds
- often exist as gases
- have low boiling points as liquids
- low melting points as solids
