Anything
how do you use a set of emission line spectrums to identify an unknown element?
The lines of the unknown element will match the lines of the given emission line spectrums.
Please explain why we can see light using: Electrons, electromagnetic radiation, excited states, ground state, and certain.
An atom will absorb and then emit energy which corresponds to wavelengths of electromagnetic radiation. This process causes electrons to move from ground state to an excited state and back again. A spectrum proves that electrons can only occupy certain energy states.
Which Color on the visible spectrum corresponds to the lowest amount of energy? How do you know? Which has the lowest and how do you know?
Lowest amount = Red .... Longest wavelength = lowest energy
Highest amount = Violet .... Shortest wavelength = highest energy
All are solid at room temperature
all have "semiconducting" properties
all have properties of elements in both other categories
All are metalloids
How would you find the energy of a photon released?
Subtract energy levels
How would you then identify the color?
a higher emission (difference) = shorter wavelength and higher energy
When assigning electrons in orbitals, each electron will first half-fill all the orbitals of the same energy before pairing with another electron in a half-filled orbital is known as:
Hund's rule
Which of the following states that electrons enter orbitals of lowest energy first?
Aufbau Principle
If two electrons occupy the same orbital they must have opposite spins is known as:
Pauli Exclusion
What are the three trends on the periodic table that we discussed in class?
Atomic Radius, Electronegativity, and ionization energy.
How would you decide which elements has a smaller atomic radius?
By looking at their location on the periodic table and using the trend
Which has the smaller atomic radius?
Na or Si
F or Cl
Be or N
Li or Rb
Si
F
N
Li
Why do nonmetals have a HIGHER ionization energy than metals?
The atomic radius is smaller, so the attraction is higher making it harder to remove electrons.
Ionization energy
amount of energy needed to remove an e- from a neutral atom
Atomic radius
distance between the nucleus and the outermost shell of an atom
Electronegativity
the ability for an atom to attract an e- from another atom + form a bond
Rank the following from least to greatest electronegativity: K, Mg, Sn, P, O
K<Mg<Sn<P<O
Group Names for 1, 2, 3-12, 17, 18
1: alkalai metals 2:alkaline metals 3-12: transitional metals 17: halogens 18: noble gasses
Which type bond is strongest and which is weakest?
Strongest: ionic
Weakest: Non-Polar Covalent