Download periodic-data-and-trends-assign-2016

GraphingPeriodicTrends
ThePeriodicTableisarrangedaccordingtoPeriodicLaw.ThePeriodicLawstatesthatwhenelementsarearrangedin
orderofincreasingatomicnumber,theirphysicalandchemicalpropertiesshowaperiodicpattern.Thesepatternscanbe
discoveredbyexaminingthechangesinpropertiesofelementsonthePeriodicTable.Thepropertiesthatwillbeexamined
inthislessonare:atomicsize,electronegativity,andionizationenergy.
Procedure
1.Useexcel(office365)orasimilarprogramtocreate3graphs(scatterplot–straightlinkconnectionsbetween
datapoints).Givethegraphanappropriatetitleandlabeltheaxes(thex-axisis‘atomicnumber’forallgraphs).
2.Cutandpastethegraphsontoaworddocumentsothattheirx-axesareinline.
3.Label/high-lightthedatapointswiththesymbolofeachalkalimetal,halogenandnoblegas.
4.Useyourgraphstocompletetheanalysisquestions(typeyourresponseinadifferentcolour!).below.Post
your completed assignment to your edublog (2 students may post identical assignments) using the tag:
mstilsnerchem11coop
1. DataTable ANALYSISQUESTIONS:usetheperiodictablebelowtosummarizethefollowingtrends.
1. Based on your graphs, what is the trend in atomic radius across a period? Down a family?
Observing the Atomic Number Vs. Atomic Radius graph the Alkali metals have a noticeably greater atomic
radius then the other elements. Also, the noble gases have a substantially smaller atomic radius then all the
other elements. The halogens also have a small atomic radius although not as small as the noble gasses.
2. Based on your graphs, what is the trend in ionization energy across a period? Down a family?
Observing the Atomic Number Vs Ionization energy graph we see that the noble gases have the highest
ionization energy. The Alkali metals have the least amount of ionization energy. Halogens Have a high
ionization energy but not as high as the noble gases.
3. Based on your graphs, what is the trend in electronegativity across a period? Down a family?
While we observe the Atomic Number Vs electronegativity graph we see that the Halogens are the most
electronegative because they have 7 valance electrons. The noble gases however have NO
electronegativity because their outer valance shell is completely full. All the Alkali metals on the graph have
are a 1 on the electronegativity Pauling scale.
4a) What is happening to the number of protons and the number of energy levels as you move across the
periodic table from left to right? How and why does this affect atomic radius.
As we move along the periodic table we see that the radius of the atom get’s smaller and smaller and hold
the electrons tighter to the protons. On the very far left the elements want to get rid of an electron and on
the far right of the periodic table the elements want to take an electron.
b) What happens to the number of energy levels as you move down a column on the periodic table. How
and why does this effect ionization energy?
The energy level gets higher/ stronger. We see on the ionization graph that the halogens for each higher
energy level the element isn't as ionized as the element in a lower energy level.
c) What happens to the effective nuclear charge as you move across a period on the periodic table? How
does this effect ionization energy and electronegativity?
The nuclear charge becomes negative, this makes the elements on the far right (the halogens and noble
gasses) have more electronegative and have a higher ionization.
5a) Which group contains elements which are easiest to ionize? Explain why this is the case.
The Alkali metals are the easiet to ionize because they only have one valence electron but also they don't
have a ton of protons compared to other elements.
b) Explain why the third ionization energy of Ca would be much higher than the 1st and 2nd ionization
energy Ca
Because the repulsion forces are a lot stronger and hold the atoms in closer to the protons.
6. Which element would have the highest electronegativity in each set below? Explain why this is.
a) Ca, Be or Mg
Be (Beryllium) would because it is the smallest atom out of the three elements.
b) B, Li, or F
F would (Fluorine) because it has the highest electronegativity because it only has one more spot in it’s
outer shell to fill.
7. Write (or type) the electron configuration of each atom (high-light the valence electrons) and it’s
corresponding ion below each sketch (atomic radii are given in angstroms (1 x 10-10 M).
(He)2S^2 3D^3
(He)2S^2 3D^6
(He)2S^2 3D^4
(He)2S^2 3D^6
(He)2s^2 3D^5
(He)2S^2 3D^6
(Ne)2S^1
(Ne)2S^2
(Ne)2S^2 2P^1
(Ne)
(Ne)
(Ne)
9. Over the blank periodic table provided, write or type the number of valence electrons and the expected ion
charge for the transition metal block and for the families to the left and right of the transitions metals (the alkali
metals have been done as an example).
Note: Carbon and boron do not normally form ions and are thus blanked-out
# valence e:
1
Ion charge:
+1