Unit 1 Flashcards
(38 cards)
What are quantum numbers
a set of 4 numbers that identifies each electron within an atom-n, I, MI, MS
Pauli’s exclusion principle?
No two electrons can have the same quantum numbers (one up one down)
What is aufbau’s principle
Start from the 1s orbital and go up while completing energy level diagrams
What is Hund’s Rule
To fill orbitals with similar energy before starting to pair electrons
What is the exception to the Cu and Cr columns in D Block
the D shell must always be half full or completely full by moving an electron from another shell (Usually S)
What are the rules for transition metals?
Never touch P orbital
How do like atoms share electrons in covalent bonds
Equally share
What is electronegativity
The relative ability for atoms to attract electrons
What are the stages of the flame test and what happens
Before the flame test, the atom is at its ground state and nothing is happening. during the flame test, the atom is excited and absorbs the energy of the flame, after the flame test, the atom is returning to its ground state and during that process light of a certain wavelength is emitted.
What is the pattern between wave length and energy
As wavelength of light increases, energy decreases and vice versa
What conclusion can be made on the electromagnetic spectrum
Based on the visible aspect of the spectrum, radiowaves (found on the left side of the spectrum) have the lowest energy but the longest wavelengths and gamma waves (found on the right) have the highest energy and the shortest wavelength.
Why are different colours seen in different cation flame tests
the difference in the wavelength emitted from the atom when excited
What are the two types of intermolecular forces
Dipole-Dipole and London Dispersion Forces
What is hydrogen bonding
A type of Dipole-Dipole force that relies on the bonding of a hydrogen atom to one of: O, N, F of another polar molecule.
What molecules are london dispersion forces in between?
Between All Atoms/Molecules
What is happening in Dipole-Dipole Attraction
As electronegativity gives molecules oppositely charged poles, when these molecule come together to create a bigger compound, they arrange themselves in a way that maximizes attractive forces and minimizes repulsive forces (-ve attracts +ve)
Types of Dipole-Dipole
Instantaneous Dipole, Hydrogen Bonding, Ion Dipole
What is an instantaneous Dipole
Molecules with temporary dipoles can induce a dipole in a nearby molecule because of its charged properties at that instant, only 1% as strong as covalent or ionic bonds
What is key about hydrogen bonding
Strongest dipole-dipole force as well as in general for intermolecular forces, binds only to O, N, or F, because of their high electronegativities
What happens to boiling point of a molecule held by hydrogen bonds
Strong forces increases BP
What can be said about the relative strength of London Dispersion forces
Increase with size of molecule, however are not strong in general. More electrons and protons means stronger force
What are Ion Dipole Forces
Forces typically found in aqueous solutions of ionic compounds, such as salt water. strongest intermolecular force
What is interesting about london dispersion forces
Occurs in all molecules non polar or polar
What is viscosity
The resistance to flow. Stronger antiparticle forces, means more viscous liquid
