Final Study Guide Flashcards
How is the concept of energy defined?
The ability to do work
What does temperature measure?
The average kinetic energy of particles in a sample of matter
What is exothermic?
When a substance GIVES OFF heat
What is endothermic?
When a substance ABSORBS heat
How many s orbitals can occupy any given energy level?
2
How many p orbitals can occupy and given energy level?
3
How many d orbitals can occupy and given energy level?
5
How many f orbitals can occupy and given energy level?
7
How many electrons can occupy an orbital?
2 electrons per orbital
What is the shape of a p orbital?
dumbbell shape
What is the shape of a s orbital?
spherical shape
Which is the lowest energy level that can have a p orbital?
Level 2
Which is the lowest energy level that can have a d orbital?
Level 3
Which is the lowest energy level that can have a f orbital?
Level 4
Is it possible for two electrons in the same atom to have exactly the same set of quantum numbers?
No, no two electrons have the same quantum numbers
When is an electron configuration considered stable?
When the subshells (orbitals) are full - like the noble gases
Describe an atom in its ground state.
An atom in its ground state has the lowest possible energy.
Describe an atom in its excited state.
An atom in its excited state has gained energy
What happens when a photon of light is emitted?
A photon of light emits when an electron goes from its excited state back to ground state
On the periodic table which direction does ionization energy increase?
Ionization energy increases as you move from bottom to top and from left to right. Fluorine has a very high ionization energy, Fr has a very low ionization energy
What is electronegativity?
Electronegativity is the ability of an atom to attract electrong
Does electronegativity increase or decrease as the atomic number of an element increases within the same period of the periodic table?
Electronegativity increases as atomic number increases. It increases from left to right across the periodic table
