Module 2, Atoms And Moles Flashcards
Isoelectronic
When ions of different elements have same number of electrons
Relative atomic mass
Average weighted mass of all isotopes of an element
How to calculate Ar of element
Ar= (% of isotope X x isotopic mass of X) + (% of isotope Y x isotopic mass of Y) / 100 . The more information/isotopes of element the more brackets.
Naturally occurring potassium consists of k-39 and k-41. Calculate percentage of each isotope present if Ar is 39.1
- 39.1=(X x 39)+(100-X)x41)/100. 2. Then x100. 3. 3910=39x+4100-41x. 4. -4100. 5. -190=39x-41x. 6. -190=-2x. 7. 95=x. K-39=95%. K-41=5%
The relative atomic mass of neon is 20.18. It consists of 3 isotopes, Ne-20, Ne-21, Ne-22. It contains 90.5% Ne-20. Find percentage composition by mass of the other 2 isotopes in neon.
- 20.18=(90.5 x 20)+(21 x X)+(22x(9.5-X))/100. 2. 20.18=1810+21X+209-22X/100. 3. X100. 4. 2018= 1810+21X+209-22X. 5. -209. 6. 1809=1810+21X-22X. 7. -1=-X. Ne-21=8.5%. Ne-22=1%
What do the peaks represent in mass spectrometry
Different isotopes
What is avogadro’s constant
6.022x10^23
What is the equation for number of particles
N(moles) x Na(avogadro’s constant)
How many atoms are there in 3 moles of water molecules
H2O= 3 atoms. 3x3x6.022x10^23=5.4198x10^24
What is the equation for number of moles
Mass(g)/mr
Calculate number of moles of c atoms and o atoms in 11g of carbon dioxide.
11/44=0.25 number of moles. CO2. C=0.25. O=0.5
Empirical formula definition
Simplest whole number of ratio. Of atoms/ions of an element in a compound.
Aluminium bromide is formed from 0.51g of aluminium and 4.49g of bromine. Calculate aluminium bromides empirical formula.
Calc moles. Ar 0.51/27=0.0189. Br 4.49/80=0.0561. Divide by smallest /0.0189. 1:2.97. 1:3. AlBr3
Work out molecular formula of NH2, given empirical and Mr= 32
N has 14 Mr and H has Mr of 1= NH2=16. 16x2=32. X ratio by 2. =N2H4
Find simplest whole number ratio for, 1:1.33
X3 so that 1.33 becomes 3.99 which round to 4 so ratio becomes 3:4