Ch301 Unit 1 Test Ep9-11 Flashcards
(42 cards)
Pauli Exclusion Principle
No 2 e- in an atom have the same 4 quantum numbers
Aufbau principle
Electrons fill from lowest E to highest E orbitals
Hunds Rule
Electrons fill degenerate orbitals singly before pairing up
Diamagnetic
An atom with all paired electrons
What type of element in the first group
Alkali metals
What type of metal is in the second group?
Alkali earth metal
What type of metal is found in d block?
Transition metals
What type of element is found in group 7
Halogens
What type of lament is found in group 8 of the periodic table
Noble gases
Radial distribution
The closer the negative electron is the positive nucleus, the stronger the electrostatic attraction, and the lower the E
Atoms achieve greater stability when
Their subshells are completely full or half full
Anytime you do econfig of ions in d orbital what needs to happen
You need to reorder the numbers in number order then remove e- from the right to the left
Do all e- in atom feel same strength of attraction to nucleus?
No the e- in a lower E level feel a stronger attraction to the nucleus
As you move across a row what happens to Zeff
Gets larger cuz more VE
How do they measure atomic radius
Distance between 2 nucleus when they next to each other because you can’t measure atomic cloud because it isn’t strictly defined
Atomic radius trends
Decreases L to R
Increases down
Positive ions are bigger or smaller than regular
Smaller
Negative ions are bigger or smaller than regular
Bigger
what is IE
The amount of E required to remove the first e- from a neutral atom in the gaseous state
IE vs work function
IE is the removal of an electron from a single gas phase atom vs the electron from a single gas phase atom
Equations for first IE
X(g) + e- -> O-(g)
EA
The change in E when an e- is added to a gaseous atom to form an anion
EA values are positive
Endothermic heat being added
EA are negative
Exothermic
Heat being released
