Chemistry Unit 2 Flashcards
Principle Energy Level
(n), #1-7, #1 is closest to nucleus, #7 is farthest from nucleus
Sublevels
(s, p, d, f) 1st PEL has 1 sublevel (s), 2nd PEL has 2 sublevels (s, p), 3rd PEL has 3 sublevels (s, p, d), 4th-7th PELs have 4 sublevels (s, p, d, f)
How many orbitals do s, p, d, and f have?
s has 1 orbital, p has 3 orbitals, d has 5 orbitals, f has 7 orbitals
Every orbital holds a maximum of _ electrons
2
Pauli Exclusion Principle
Both electrons in the orbitals have opposite spins
Aufbau Principle
Electrons are placed in the lowest energy level possible
Hunds Rule
Every orbital within a sublevels gets one electron before any orbital in that sublevel gets two
Valence Electrons
Electrons in the highest PEL, used in bonding, first lost when forming ions, 8 is the maximum, always come from s and p sublevels
Copper Electron Configuration
1s2 2s2 2p6 3s2 3p6 4s1 3d10
Chromium Electron Configuration
1s2 2s2 2p6 3s2 3p6 4s1 3d5
How many valence electrons does chromium have?
1
Excited State
When an element absorbs energy the electrons can jump to a higher energy level must be the exact amount of energy
When is energy given off in the form of light?
When electrons emit energy and fall back from the excited State to the ground state
High energy = ____ wavelength and ____ frequency
Short wavelength and high frequency
Low energy = ____ wavelength and ____ frequency
High wavelength and low frequency
Wavelength
The distance between 2 peaks or troughs (in meters)
Frequency
How often waves pass a given point (in s-1 or Hertz)
Wavelength and frequency have a(n) ____ relationship
Inverse
Continuous Spectrum
Shows all the wavelengths of visible light
Absorption Spectrum
A continuous Spectrum with black lines that represent the energy that was absorbed by an electron to transition between levels
Emission Spectrum
Shows the energy of the light being emitted as the electrons fall back down (black bar with colored lines)
What do the lines do in a hydrogen emission spectrum?
Lines converge at higher energy
Lyman Series
When electrons fall to n=1, they give off ultraviolet light
Balmer Series
When electrons fall to n=2, they give off visible light
Paschen Series
When electrons fall to n=3, they give off infrared light
The longer the arrows on absorption/emission spectrums, the ____ energy is being absorbed/emitted
The more energy
What is z equal to?
The atomic number
Different isotopes have ____ chemical properties and ____ physical properties
The same chemical properties and different physical properties
If there is a large jump in the ionization energies, that indicates a ____
Change in principle energy level, or that all valence electrons are lost
What does isoelectronic mean
The same number of electrons
The plane of px orbitals is at __ degrees to the planes of py and pz orbitals
90 degrees
True or False: Atoms of the same element are alike in every way
True! This was discovered by Dalton
Thomson used _____ rays to conclude that atoms contain very small, negatively charged particles called electrons
Cathode
What type of particles did Rutherford aim at gold foil?
Alpha particles
Rutherford found that the core atom is _____
Dense
Bohr found that atoms are held together by _____ force between a positive nucleus and negative surroundings
Electrostatic Force
Where in the data booklet can you find the actual mass of a proton, neutron, and electron?
Page 3!
What is a nucleon?
The protons and neutrons in the nucleus
What are the units for relative atomic mass?
There aren’t any, it’s relative!
Atomic Mass
The weighted average of all naturally occurring isotopes for an element
Mass Number
The sum of the protons and neutrons in an element
Isotopes always have …
The same number of protons and a different number of neutrons
What goes on the x-axis in a mass spectrum?
Mass/Charge
What goes on the y-axis in a mass spectrum?
Abundance
What four processes occur inside a mass spectrometer (in order)?
- Ionization
- Acceleration
- Deflection
- Detection
In a mass spectrometer, what is ionization?
Electrons are knocked off sample particles to form (mostly) +1 ions
In a mass spectrometer, what is acceleration?
Ions move through a series of charged plates to form a narrow beam of high speed particles with equal kinetic energy
In a mass spectrometer, what is deflection?
Ions are attracted to the negative side of an electromagnetic field, causing separation of the mixture based on mass and charge
In a mass spectrometer, what is detection?
Ions collide with a metal plate. Electrons are transferred from the metal to the ion, producing a current and thus a signal to the computer
In a mass spectrometer, lighter ions go to the (inside/outside), heavier ions go to the (inside/outside), and where do the middle ions go?
Lighter - inside
Heavier - outside
Middle - down the middle
In a mass spectrometer, greater deflection means a ____ turn towards the negative pole of the electromagnet
Tighter
Mass spectroscopy is sorting based on what?
Mass
Why do the sum of all relative intensities in mass Spectra not equal 100?
The first ion to hit the detector in the mass spectrometer is automatically given a relative intensity of 100, and the others are given based on their proportion to the first one
What physical properties are different in different isotopes of the same element?
Mass number, melting or boiling point, density, freezing point
What isotope are all atomic masses relatively measured to?
Carbon-12
What phase of matter does ionization energy remove one mole of electrons from?
The gaseous phase
What does A mean?
Atomic mass
