Question

Explain why vanadium (radius = 134 pm) and copper (radius = 128 pm) have nearly identical atomic radii, even though the atomic number of copper is about 25% higher than that of vanadium. What would you predict about the relative densities of these two metals? Look up the densities in a reference book, periodic table, or on the Web. Are your predictions correct?

Answer 1

is this one whole question

Answer 2

yes

Answer 3

@Secret-Ninja @Compassionate

Answer 4

ugh help :(

Answer 5

this one i don't know sorry

Answer 6

there are few main factors affecting the atomic radii, the outermost electrons and the protons in the nucleus, also the shielding of the internal electrons.
I would speculate that the difference in radii is given by the electron clouds. Since the electrons difference in these two elements are in the d orbital and both has at least 1 electron in the 4s (this 4s electron is the outermost electron in all the transition metals of this period). Then the atomic radio will be mostly dependent of these 4s electrons than in the d electrons.
Besides that you can see that increasing the atomic number will increase the number of protons in the nucleus decreasing the radio of the atoms along a period. The Cu is an exception will accomodate one of the 4s electrons in the p orbital to

Answer 7

is your prediction correct @Cuanchi

Answer 8

have you finished your entire answer?

Answer 9

What do you think? what is your prediction? you have any objection?

Regarding to the density you can find the density for Cu=8.96g/cm3 and vanadium =6.0g/cm3 this also correlate with the idea that if these two atoms have similar volume and one has more mass (more protons), density is the relationship between m/V, then a bigger mass for a similar volume will result in a bigger density

Answer 10

thank you !!