1. Metal Reactivities Lab – Introduction
investigate the relative reactivity (tendency to ______________)
of eleven metals
if atoms of elements are reactive,
they react with other _____________________
to form _______________________
*****KEY*******
(relatively) reactive metals tend to be ________________________
(relatively) unreactive metals tend to be ______________________
chchchchange
elements
compounds
in compounds
pure

2. metal atoms lose OR gain electrons when they react with nonmetals
(the nonmetal atoms lose OR gain electrons)
**KEY** so,… in compounds, the metal is found as a _________________________
the nonmetal is found as a ______________________
example: pure sodium – Na and pure chlorine – Cl
react to form the
compound sodium chloride
Na Cl Na+ and Cl- (or NaCl)
positive ion (cation)
negative ion (anion) e-

3. metal atoms lose OR gain electrons when they react with nonmetals
(the nonmetal atoms lose OR gain electrons)
(lose/gain enough electrons to get a _______________)
**KEY** so,… in compounds, the metal is found as a _________________________
the nonmetal is found as a ______________________
predict the easier / harder it is to lose electrons the more / less reactive the metal
the easier / harder it is to gain electrons the more / less reactive the nonmetal
full outer shell
positive ion (cation)
negative ion (anion)
METALS
NONMETALS
MOST
LEAST
LEAST
MOST

4. Li, Na, K, Mg, Ca, Fe, Cu, Ag, Zn, Al, and Pb
METALS
NONMETALS
MOST
LEAST
LEAST
MOST
you will carry out a series of reactions to establish the relative reactivity of the eleven metals
Li, Na, K, Mg, Ca, Fe, Cu, Ag, Zn, Al, and Pb
then, you will compare what you observe experimentally to
what you would predict based on trends
AND
offer explanations for deviations of the observed reactivity from the predicted reactivity

5. PART A – Ag, Cu, Fe, Zn, Pb
Test the relative reactivities of these metals based on the principle that
the more reactive metal will tend to be in a compound OR pure
the less reactive metal will tend to be in a compound OR pure
Example: Copper (Cu) and Zinc (Zn)
Cu(SO4) (aq) Zn (s) observe
Zn(SO4) (aq) + Cu (s) observe
focus on
Cu(SO4) (aq) Zn (s)
copper in a compound
pure zinc
pure copper
zinc in a compound
the change (reaction) happens, because
copper “prefers” to be ______ _____________________
and zinc “prefers” to be ____________ __________________
pure
copper is less reactive
in a compound
zinc is more reactive

6. Cu(SO4) (aq) + Zn (s) Cu (s) + Zn(SO4) (aq)
copper in a compound
the less reactive metal
ends up pure
pure zinc
the more reactive metal
ends up in a compound
pure copper
zinc in a compound
the change (reaction) happens, because
copper “prefers” to be pure _____________________
and zinc “prefers” to be in a compound ___________________
copper is less reactive
zinc is more reactive
this type of reaction is called single displacement
a more reactive element displaces a less reactive element from a compound
(the two elements swap being pure / in a compound)
this type of reaction is the basis of some batteries…..

7. Single displacement reactions and batteries
Cu(SO4) (aq) Zn (s) Cu (s) + Zn(SO4) (aq)
copper in a compound
zinc in a compound
the less reactive metal
ends up pure
the more reactive metal
ends up in a compound
pure zinc
pure copper
Cu2+
Zn2+
when pure metal atoms react, they lose electrons cations of the metal in a compound
Cu loses 2 e Cu2+
Zn loses 2 e Zn2+
for a metal cation in a compound to become a pure metal atom, the cation must gain electrons
Cu2+ gains 2 e Cu
Zn2+ gains 2 e Zn
Zn Cu
2e-
Zn Cu2+

8. Phew… right….. so,….. for PART A
principle – the more reactive metal “wants” to be in a compound
the less reactive metal “wants” to be pure
to test for the relative reactivity of two metals,
- start with one pure and one in a compound
- combine
- look for evidence of the “swap” (single displacement)
key evidence
set up looks like….

9. PART B and C – (also) Single displacement reactions
Test the relative tendency of a metal to displace hydrogen from a compound
PART B – Mg, Zn, Pb, Al
example: Mg (s) + HCl (aq) ??  ?? H2 ( ) +
evidence ? _________________
PART C – Li, Na, K, Ca, Mg
example: Mg (s) + H2O (l) ??  ?? H2 ( ) +
(hydrogen is acting like a metal)
BUBBLES
BUBBLES
In either part (reacting with HCl / H2O) how can you tell which metal is MORE reactive?

10. Metal Reactivities Lab – Postlab
metal atoms lose OR gain electrons when they react with nonmetals
(the nonmetal atoms lose OR gain electrons)
**KEY** so,… in compounds, the metal is found as a _________________________
the nonmetal is found as a ______________________
Reactivity (of metal atoms) depends on:
1. _____________________________
which depends on ____________________________________________
2. _____________________________
to get ______________________________________________________
cationx+
aniony-
opposite charges attract (bond)
compound
positive ion (cation)
negative ion (anion)
how easy it is to lose electrons (IE)
atomic size (and sublevel configuration)
# of electrons to lose
a FOS (or full or ½-full sublevel)
combination of these two gives ________________________
the lower this value, (predict) the ____________ reactive
total IE
MORE

11. silver Ag copper Cu zinc Zn
METALS
NONMETALS
MOST
LEAST
LEAST
MOST
silver Ag copper Cu zinc Zn
predict ____________________________________
observe ___________________________________
so,…. there must be something else going on other than
______________________________
Ag more reactive than Cu more reactive than Zn
Zn more reactive than Cu more reactive than Ag
hmmmmmmm……….
how easy it is to lose electrons
total IE
# of electrons to lose to get FOS
(or some other stable e- configuration)

12. silver Ag copper Cu zinc Zn
predict ____________________________________
observe ___________________________________
so,…. there must be something else going on other than
______________________________
Ag more reactive than Cu more reactive than Zn
Zn more reactive than Cu more reactive than Ag
hmmmmmmm……….
how easy it is to lose electrons
total IE
# of electrons to lose to get FOS
(or some other stable e- configuration)
***KEY*** _________________________________
but, by definition, _____________________________
there must at least be __________________________
for ISOLATED atoms
a reaction cannot happen with an ISOLATED atom
at least two atoms to react
well let’s consider what happens when an isolated atom
becomes un-isolated….

13. isolated atom
isolated You
to the chalkboard…..

14. silver Ag copper Cu zinc Zn
predict ____________________________________
observe ___________________________________
so,…. there must be something else going on other than
______________________________
Ag more reactive than Cu more reactive than Zn
Zn more reactive than Cu more reactive than Ag
hmmmmmmm……….
how easy it is to lose electrons
total IE
# of electrons to lose to get FOS
(or some other stable e- configuration)
***KEY*** _________________________________
but, by definition, _____________________________
there must at least be __________________________
for ISOLATED atoms
a reaction cannot happen with an ISOLATED atom
at least two atoms to react
*****KEY***** any other “stuff” around will influence
the behavior (reactivity) of the atom(s) of interest
what other “stuff” is around?

15. especially the presence of water
Environmental Factors and Metal Reactivity
ex: Copper vs Silver
observe: ____________ is more reactive than _______________
predict:
based on atomic size _________________________
because ______________________________________________
based on # of electrons to lose _______________________
Ag loses _________ ____________
total IE = 1st IE = __________________
Cu loses __________ ____________
total IE = 1st IE + 2nd IE = ___________________
BUT…..
so, ______________________________________________
predictions are based on ___________________________
for a reaction to occur ____________________________________________
______________________________________________________________________
copper
silver
silver more reactive than copper
(trends) silver atoms larger than copper
silver more reactive than copper
1 e-
Ag+
733 kJ/mol Ag
total IE
2 e-
Cu2+
2712 kJ/mol Cu
there must be some other factor(s)
single, ISOLATED atoms
can’t be… need (at least) two atoms
especially the presence of water
the presence of any other substance, the Temperature, the pressure,…
(the environment) all effect the reactivity of atoms

16. Cu (s) + 2 Ag(NO3) (aq) 2 Ag (s) + Cu(NO3)2 (aq) H** **
Cu (s) Ag(NO3) (aq) Ag (s) Cu(NO3)2 (aq) H O H O H O H O
metal in
a compound
must be a(n)
_________
Ag+
Cu2+
(NO3)- H O
(NO3)-
(NO3)- H O
cation H O
so nitrate
must be a(n)
__________ H O
anion
water is ___________ the O side is slightly (-) so, sticks to _________________
the H side is slightly (+) so, sticks to ________________
water will stick more tightly to ions that have higher or lower charge
Cu2+ OR Ag+
water will stick more tightly to ions that are smaller or larger
STICKY
cations
anions

17. to unstick (____________) ______________________________________
so,
to stick (_______________) must _______________________________________
so, when water sticks to a metal cation,
the cation (and water) become more _____________
so, water stabilizes _________ AND water stabilizes ________
stabilize = __________________________
so, ______________________________________
which is the same as saying water encourages the ____________ to form
which is the same as saying water encourages the metals to ____________
so, __________________________________________________________
pull apart
takes energy
so, becomes less stable
come together
release energy
so, becomes more stable
stable
Cu2+
Ag+
(because water
sticks to them)
metal cations
= metals in ___________
compounds
encourages to happen
water encourages the cations to form
compounds
react
water increases the reactivity of ALL metals
reactivity
metals in the
presence of water
pure metals

18. water increases the reactivity of ALL metals
metals in the
presence of water
pure metals
water sticks more tightly to Cu2+ OR Ag+ ?
Why?
so, water _______________ the reactivity of ___________________
moreso than the reactivity of ____________________________
because,
water stabilizes the _________ cation (__________ in a ___________)
moreso than it stabilizes the _______ cation (__________ in a ___________)
copper ions are smaller and have higher charge
than silver ions
increases
(the pure metal) copper
(the pure metal) silver
copper
copper
compound
silver
silver
compound

19. water increases the reactivity of ALL metals
water _______________ the reactivity of ___________________
moreso than the reactivity of ____________________________
because,
water stabilizes the _________ cation (__________ in a ___________)
moreso than it stabilizes the _______ cation (__________ in a ___________)
increases
(the pure metal) copper
(the pure metal) silver
copper
silver
compound Cu Ag
metals in the
presence of water
reactivity
pure metals Ag Cu

20. Why is Copper more reactive than Silver ?
Cu2+ (g), 2 Cl (g)
1st + 2nd IE Cu
(1st EAE Cl)  2
Why is Copper more reactive than Silver ?
Cu2+ (g), 2 Cl- (g)
the presence of chlorine (chloride)
influences the stability of the product
therefore the reactivity…
the presence of water
influences the stability of the product even more
therefore the reactivity even more…
Ag+ (g), Cl (g)
1st EAE Cl
1st IE Ag
Ag+ (g), Cl- (g)
Cu (g), 2 Cl (g)
isolated
atoms
isolated
atoms
Ag (g), Cl (g)
Ag+Cl- (aq)
Ag (s), ½ Cl2 (g)
Cu (s), Cl2 (g)
Cu2+Cl2- (s)
Ag+Cl- (s)
Cu2+Cl2- (aq)

21. The environment (temperature, pressure, and any other “stuff”)
affects the reactivity of metals (or any substance)
**especially the presence of water
Water sticks to cations (metal ions in compounds)
so, water stabilizes the metal _____________________
and therefore, ___________________ the reactivity
(of all metals above the reactivity w/o water present).
Water will increase the reactivity to a greater degree for metals that form
_____________ and _______________________ cations
in a compound
increases
smaller
more highly charged

22. most reactive nonmetals smallest atoms - easiest to gain e-
Summary of Trends
across a period
atoms get smaller
ions get smaller
down a group
atoms get larger
ions get larger
to get a FOS
# e- to lose
# e- to gain
more
less
same
most reactive nonmetals
smallest atoms
- easiest to gain e-
fewest e- to gain
to get a FOS IE
harder to lose e-
easier to gain e-
EAE
metals
nonmetals
most reactive metals
(aside from noble gases)
least reactive
largest atoms
- easiest to lose e-
fewest e- to lose
to get a FOS IE
easier to lose e-
harder to gain e-
EAE

23. the reactivity of these metals more
Summary of Trends
across a period
atoms get smaller
ions get smaller IE
so,… water increases
the reactivity of these
metals more
EAE
to get a FOS
# e- to lose
metals
nonmetals
more
less
most reactive metals
form
smaller ions
higher charge
(aside from noble gases)
least reactive
form
larger ions
lower charge
down a group
to get a FOS
atoms get larger
than it increases
the reactivity of
these metals
ions get larger
# e- to lose
same IE
EAE
opposite the trend for reactivity
for isolated atoms !

24. Why is Copper more reactive than Silver ?
Cu2+ (g), 2 Cl (g)
1st + 2nd IE Cu
(1st EAE Cl)  2
Why is Copper more reactive than Silver ?
Cu2+ (g), 2 Cl- (g)
Ag+ (g), Cl (g)
1st EAE Cl
1st IE Ag
Ag+ (g), Cl- (g)
Cu (g), 2 Cl (g)
isolated
atoms
Ag (g), Cl (g)
isolated
atoms
Ag (s), ½ Cl2 (g)
Cu (s), Cl2 (g)