Exam Q 2 Flashcards
What is an electron?
It is a negatively charged subatomic particle that orbits an atomic nucleus.
Why might the electron in a hydrogen atom not occupy the n=1 energy level?
It is in an excited state/gained energy/absorbed a photon
What colour light is associated with the electron in a hydrogen atom moving from n=3 to n=2
red
Name the series of lines visible in the hydrogen emission spectrum
Balmer Series
How many sub levels are associated with the n=3 energy level?
3
What is an atomic orbital?
It is the region in space within which there is a high probability of finding an electron
Write electron configuration for beryllium, neon and krypton
1s^2, 2s^2
1s^2, 2s^2, 2p^6
1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 3d^10, 4s^2, 4p^6
How many orbitals are associated with the n=2 energy level?
4
a single 2s orbital, and three orbitals labeled 2p
What is the maximum number of electrons that can occupy the n=3 energy level in a multi-electron atom?
18=2+8+8
Why are the elements krypton and neon chemically inert?
They have stable full outer octet (ns^2 np^6) electrons
/
8 electrons in outer shell (energy level) is stable
Why are the elements beryllium and magnesium reactive?
They do not have stable full outer octet (ns^2 np^6) electrons
/
do not have 8 electrons in outer shell (energy level) is stable
Why is the element magnesium more reactive than beryllium?
Mg has a greater atomic radius, it has more energy levels
outer electrons of Mg are further from nucleus
