# How does density of alkali metals increase down the group?

Size of alkali metals increases down the group, so volume also shows increment, and since volume is inversely proportional to density, how does density also increase down the group?

• Because mass is also increasing, presumably faster than volume. – ringo Feb 20 '17 at 15:49
• Do you mean "why"? "How" suggests you may want to know whether the increase is linear or some other mathematical function. – bpedit Feb 20 '17 at 16:10
• The molar volume increases from 13.10 cm$^{3}$/mol for Li to 71.07 cm$^{3}$/mol for Cs. Mass increases from 6.9 gm/mol for Li to 132.9 gm/mol for Cs. So, the mass per atom increases faster than the atomic density decreases. – Jon Custer Feb 20 '17 at 17:05

## 3 Answers

$Density=mass/volume$

1) If mass is increasing and volume is decreasing, then density (mass/volume) will increase.

2)If mass is decreasing and volume is increasing simultaneously, then the density (mass/volume) will decrease.

*3)If both mass and volume are increasing, then we need to check which one of them is increasing at a faster rate(since both are contradictory factors)

a) If mass is increasing at a faster rate than volume, then density will increase.

b) If volume is increasing at a faster rate than mass (i.e denominator in mass/volume is increasing making the overall fraction smaller), then density decreases.

You can apply same logic when both volume and mass are decreasing simultaneously.

Generally, we see that in alkali metals the rate of increase of mass is greater than rate of increase of volume, therefore the density increases down the group.

Also, note that there is no definite reason for why mass is increasing at a faster rate than volume. So asking "why" does it happen isn't a great question.

Its just because density is directly proportional to mass. And the mass increases faster than that of volume expect for the case of potassium which is lighter than sodium. It is the total differential of the d = m/v equation, not the equation itself, that gives you the effect of increasing row number on density. d = m/v tells you nothing about what happens to m and v as you increase the row number of the atom. Don't confuse an equation with the change in the variables in that equation as a function of something else (in this case, At. No.). There's two important effects in answering your question. First, mass increases as you increase At. No.,but it for every 1 unit increase in charge (1 proton and 1 electron), the mass increases by more than 1. (the mass of an electron is less than 1/1800th of the mass of a proton, so its mass can be ignored, as can the volume of the nucleus - its volume is negligible) As at no. increases the element, on average, requires an increasing number of neutrons to keep the atom together, and since a neutron is almost exactly the same mass as a proton, mass increase faster than at. no. Check out this graph https://en.wikipedia.org/wiki/Isotope#Nuclear_properties_and_stability and note that almost all of the stable isotopes are above the neutron/proton = 1 = Z/N line, meaning there is more than 1 neutron to each proton (on average). Note also the curve in the distribution of stable elements. So, mass increases faster than at. no. - what about volume? It turns out that the valence electron determines an element's atomic (covalent) radius. It turns out that all the electrons are held closer in towards the positively charged nucleus as the charge on the nucleus increase (as at. no. increases). There's a couple of reasons for that. One is that the repulsion between electrons as you add an electron to the atom isn't as strong as the attraction between all the electrons and the additional proton. Another way to explain it is that volume increases as the 3rd power of radius,which can be thought of to mean that a little increase in radius gives the electrons a lot more room, so that they're not going to push that valence electron too far out from the nucleus. Another way to explain this is the fact that the inner electrons are not 100% efficient at shielding outer electrons from the nuclear charge (pretty obvious, right? I mean if they were 100% efficient then you'd expect the outer electrons to wander away...) So, each added inner electron doesn't "cancel" each added protons charge as felt by the valence electron, that is it doesn't fully, 100% cancel the attraction. All this means size increases slower than mass (in a given period). Note that going across a row requires a more detailed (quantum mechanical/orbital) analysis because the different orbitals (s, p, d, f, etc.) have different shielding efficiencies. Since you're considering only down the alkali metals, this doesn't have to enter in to your considerations.

• Paragraphs Li Zhi, please break your answers into more easily digested paragraphs ;) The answer above should probably be eight paragraphs. Also, I noticed that you used at least 3 slightly different means of abbreviating "atomic number". If you feel it needs to be abbreviated at all, then at least pick one and stick with it. My main comment though, is that I really think your answers will be far more readable if you just break them down into paragraphs. – airhuff Feb 20 '17 at 20:26