Question

complete the following table:
element electron config. highest e level? # valence e⁻ # of protons is it stable?
carbon
nitrogen
which atom, carbon or nitrogen, has the smaller radius? why?

1. arrange the following in order of decreasing size:

e. sr, i, ag, mo
f. ge, si, sn, c
g. al, he, cs
h. cl, na, ar, p

1. arrange the following in order of increasing force of attraction between valence electrons and the nucleus:

d. be, ba, ca
e. n, o, f, li
f. kr, xe, ne

Explanation:

Step1: Determine electron - config, highest E level, valence e⁻, protons and stability for Carbon

Carbon has an atomic number of 6.

• Electron config: $1s^{2}2s^{2}2p^{2}$
• Highest E level: 2
• # Valence e⁻: 4
• # of protons: 6
• Is it stable: No (needs 8 valence electrons to be stable)

Step2: Determine electron - config, highest E level, valence e⁻, protons and stability for Nitrogen

Nitrogen has an atomic number of 7.

• Electron config: $1s^{2}2s^{2}2p^{3}$
• Highest E level: 2
• # Valence e⁻: 5
• # of protons: 7
• Is it stable: No (needs 8 valence electrons to be stable)

Step3: Compare atomic radii of Carbon and Nitrogen

Both are in the second period. As we move across a period from left to right, the nuclear charge increases while the shielding effect remains relatively constant. Nitrogen has a greater nuclear charge (7 protons) compared to carbon (6 protons), so the electrons are pulled in more tightly. So nitrogen has a smaller radius than carbon.

Step4: Arrange in order of decreasing size

e. Sr, I, Ag, Mo

Sr is in period 5, group 2; I is in period 5, group 17; Ag is in period 5, group 11; Mo is in period 5, group 6. As we move from left to right in a period, the atomic size decreases. So the order is Sr > Mo > Ag > I.

f. Ge, Si, Sn, C

C is in period 2, Si is in period 3, Ge is in period 4, Sn is in period 5. As we move down a group, the atomic size increases. So the order is Sn > Ge > Si > C.

g. Al, He, Cs

Cs is in period 6, Al is in period 3, He is in period 1. So the order is Cs > Al > He.

h. Cl, Na, Ar, P

Na is in group 1, P is in group 15, Cl is in group 17, Ar is a noble - gas in group 18 of period 3. So the order is Na > P > Cl > Ar.

Step5: Arrange in order of increasing force of attraction between valence electrons and the nucleus

d. Be, Ba, Ca

As we move down a group, the distance between the valence electrons and the nucleus increases and the force of attraction decreases. So the order is Ba < Ca < Be.

e. N, O, F, Li

As we move across a period from left to right, the nuclear charge increases and the force of attraction between the valence electrons and the nucleus increases. So the order is Li < N < O < F.

f. Kr, Xe, Ne

As we move down a group, the distance between the valence electrons and the nucleus increases and the force of attraction decreases. So the order is Xe < Kr < Ne.

Answer:

Element	Electron Config.	Highest E level	# Valence e⁻	# of protons	Is it stable?
Nitrogen	$1s^{2}2s^{2}2p^{3}$	2	5	7	No

Nitrogen has a smaller radius than carbon because it has a greater nuclear charge in the same period, pulling electrons in more tightly.
e. Sr > Mo > Ag > I
f. Sn > Ge > Si > C
g. Cs > Al > He
h. Na > P > Cl > Ar
d. Ba < Ca < Be
e. Li < N < O < F
f. Xe < Kr < Ne