Metal/NonMetal/Metalloid
Sodium
Metal
Which is more electronegative?
Al, N, or Ca
N
Which has a larger ionization energy?
Na or K
Na
Smaller Radius? K or Rb
K
Which has a larger radius?
F or F-
F-
Metalloid
Which is more electronegative?
He, Cl, F
F
Which has a larger ionization energy?
Na or Mg
Mg
Larger Radius?
Si or P
Si
Which has a larger radius?
Mg or Mg+2
Mg
Helium
Non Metal
Rank from smallest to largest electronegativity.
V, Ba, Al, Zn
Ba, V, Zn, Al
Define ionization energy
the amount of energy required to remove an electron
Rank smallest radius to largest radius.
N, Ba, Ga
N < Ga <Ba
Rank smallest radius to largest radius
C-1, C, C+1
C+1, C, C-1
Conductive
Metal
SCIENTIFICALLY, why is Mg more electronegative than Ca
must mention energy levels and distance
increased distance results in weaker coulombic attraction for the electrons in Ca
Explain the difference between the value of the first ionization energy and second ionization energy of potassium.
2nd = higher because K has 1 valence electron and removing the first electron will result in a full valence shell in which it is difficult to remove the 2nd electron
SCIENTIFICALLY, explain whether Li or Na has a larger atomic radius.
Na is larger because it has 3 energy level compared to Li's 2.
Which has the largest radius and WHY?
K or K+1
K
K+1 has lost an electron so there are more protons and less electrons. the larger amount of protons will pull the electrons in more, decreasing the radius
Not Lustrous
Non Metal
SCIENTIFICALLY, why is O more electronegative than C?
Must mention either nuclear charge or shielding
both cause the force of attraction between the nucleus and electrons to increase
Explain, using science concepts, why F has a larger ionization energy than Li
Li has 1 val e and F has 7
Removing 1 electron from Li would result in a newly full valence shell. This is not the case for F.
Also, F has a higher nuclear charge and more shielding which increases the force the nucleus has on the electrons.
SCIENTIFICALLY explain which is has a larger radius and why (Al or S)
Al
nuclear charge of Al = 13
nuclear charge of S = 16
higher charge = greater force of attraction
Sulfur's electrons are pulled in closer to the nucleus
Which is smaller and WHY?
O or O-2
O
O-2 has more electrons in the outer orbitals. These want to repel each other, so they spread out more and increase the radius.