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Atoms and the Periodic Table
Atom
Nucleus located in center of atom is small, dense and positively charged. Contains protons and neutrons
Region outside the nucleus contains electrons
Sub-Atomic Particles
Particle Mass Charge Location
(amu)
Proton 1 + 1 Nucleus
Electron 1/1835 - 1 Outside nucleus
Neutron 1 0 Nucleus
Atomic number (Z) is the number of protons in an atom
The number of protons determines the identity of the element
Mass number (A) is the total number of protons and neutrons in an atom
Atom X
Mass number Charge A C
X Z
Atomic number
X is atomic symbol
An atom has 47 protons, 61 neutrons and 47 electrons.
What is its atomic number?
What is its mass number?
What is its charge?
What element is it?
What is its atomic mass?
Ag
Mass number Charge47p + 61n 108 0 47p+ + 47 e-
Ag47 p 47
Atomic number
Ag atomic symbol
31
X 15
atomic number
mass number
number of protons
number of electrons
number of neutrons
element symbol
31
X 15
atomic number 15
mass number 31
number of protons 15
number of electrons 15
number of neutrons 31-15 = 16
element symbol P
Isotopes
Isotopes are atoms of the same element that have different numbers of neutrons
Isotopes have different masses
Isotopes of an element have the same chemical properties.
Isotope Protons Neutrons Mass # Name
12C 6 6 12 Carbon-12
13C 6 7 13 Carbon-13
14C 6 8 14 Carbon-14
C-14 is radioactive.
Radioactive isotopes have the same chemical properties as other isotopes of the same element
Atomic Mass of an Atom
Each proton and neutron has a mass of approximately 1 amu
For C-13, mass would be:
6 protons x 1amu/proton = 6 amu7 neutrons x 1 amu/neutron = 7 amu
Mass of C-13 atom = 13 amu
Atomic Mass Unit (amu)
Atomic Mass Unit is defined as 1/12 the mass of the 12C (C-12) isotope of carbon
Atomic Mass of Element
Often called atomic weight
Atomic mass of an element is weighted average of the masses of each isotope
Need to know abundance of each isotope to calculate atomic mass
Chlorine occurs as two isotopes Cl-35 and Cl-37
75.77% Cl-35 (or 0.7577)
24.23% Cl-37 (or 0.2423)
0.7577 x 35 amu = 26.52 amu
0.2423 x 37 amu = 8.965 amu
Cl Atomic mass = 35.49 amu
Calculate the atomic mass of Imaginarium
90 % occurs as Im-200
10 % occurs as Im-210
Calculate the atomic mass of Imaginarium
90 % occurs as Im-200
10 % occurs as Im-210
0.90 x 200 amu = 180 amu
0.10 x 210 amu = 21 amu
mass of “average” 201 amu
atom
Atom
Neutral atom has equal number of protons and electrons
+ charges = - charges
Overall charge of zero (neutral)
Ions
Atom can gain or lose electrons to form ion
Gain electrons → negative ion (anion)
+ charges < - charges → - ion
Lose electrons → positive ion (cation)
+ charges > - charges → + ion
Atoms are so small that we cannot easily measure distances
Can measure energy (in form of light):
Spectroscopy
Can think of entire electromagnetic spectrum as if it were light
Electromagnetic Radiation
Travels at speed of light: 3.0 x 108 m/s
Travels as waves --- Wavelength (λ) and Energy inversely
relatedSmall λ -- High energyLong λ -- Low energy
Spectrum can be divided into regions based on wavelength and energy
The Wave Nature of Light• All waves have a characteristic
wavelength, , and amplitude, A.
• The frequency, , of a wave is the number of cycles which pass a point in one second.
• The speed of a wave, v, is given by its frequency multiplied by its wavelength:
v = • For light, speed = c.
Fig. 2.10
Emission Spectrum
Pass electricity through vacuum tube that has gas phase atoms
Specific wavelengths of light are emitted
Each element emits characteristic wavelengths
Visible light spectrum is continuous
Emission spectrum is discontinuous
Only certain bands seen
(allowed energy amounts – quanta)
Fig. 2.11
Bohr Atom
• Electrons are found in “orbits” around the nucleus
• Each “orbit” is called a principal energy level (n) --- or shell
• The higher the energy level, the farther out from the nucleus it is
• The higher the energy level, the greater the energy of the electrons in it
Bohr Atom
Electrons can only have certain allowed amounts of energy
Quantum: a discrete amount of energy
Photon: a packet of energy (light)
Ground state:Electrons in lowest possible energy level
Excited state:Electron has absorbed energy and been promoted to a higher energy level (farther from nucleus)
Relaxation occurs when electron emits energy and goes into a lower energy level (closer to nucleus)
Only specific amounts of energy can be absorbed or emitted (quantum of energy)
If energy emitted corresponds to a visible wavelength, we see it as a colored line in the emission spectrum
The pattern is unique for each element
Bohr’s model worked for Hydrogen, but not for more complicated atoms (more e-)
Fig. 2.11
http://astro.u-strasbg.fr/~koppen/discharge/
• Ne red
• Ar blue
• Hg blue
• Na yellow
Principal Energy Level Element # e- 1 2 3 4
H 1 1He 2 2Li 3 2 1Be 4 2 2C 6 2 4F 9 2 7Ne 10 2 8Na 11 2 8 1Mg 12 2 8 2Cl 17 2 8 7Ar 18 2 8 8K 19 2 8 8 1