Name: __________________________________________________________ Date __________________________________ Period ___________
(Unit 5.1)
MANY ELEMENTS ARE UNSTABLE
 Many elements do not exist all by themselves in nature.
 They _____________________ with other elements and form ______________________.
 This is because their neutral form is _________________________.
 In other words, they have A LOT of chemical potential energy.
 Having a lot of chemical potential energy is like a pencil standing on its point.
 Eventually it will fall to a lower energy position.
 Everything in the universe tends towards as ____________ an energy state as possible, so elements will do what they need to do to be more _____________________.
HOW DO ELEMENTS BECOME MORE STABLE?
 Many elements are unstable because they have _____________________ electron configurations.
 The most stable electron configuration is having 8 electrons in the highest energy level (a full ______________).
 Unstable elements will ________________ or lose valance electrons to achieve a full octet.
 Then they will have an overall _____________________ and will be known as ___________________.
 Elements will gain or lose valance electrons to be like the closest _________________________ gas.
 Example: Fluorine 9p + and 9e -
 e configuration: ______________________________
 It has ______ valance electrons.
 It will gain one more electron and its electron configuration would be the same as Neon’s:
___________________________.
 It would have an overall charge of ___________. Why?_________________________________
ANIONS
 Once fluorine gains its electron it is now known as a _____________________ ion which is represented with the symbol: ____
 Negative ions like fluorine are known as _______.
 Other ___________________ like Cl and Br will also form anions with ____________ charges.
 Why? ________________________________________
 Since other non metals also have high ________________________ they will also gain electrons and form
_______________________.
 Group 16 elements will gain ______valance electrons and will end up with a _______ charge.

Name: __________________________________________________________ Date __________________________________ Period ___________
 Group 15 elements will gain __________ valance electrons and will end up with a ____ charge.
CATIONS
 ______________ tend to ___________ electrons to become stable.
 Example: Sodium 11p + and11e -
› e configuration:_________________
›
It has _______ valance electron.
›
It is easier to lose 1 valance electron then to gain _______.
›
So its electron configuration will end up the same as Neon’s: _________________.
›
It would have an overall charge of ________. Why?
 Once sodium loses its electron it is now known as a sodium ion which is represented with the symbol: ______
 Positive ions like Na+ are known as _____________.
 Other alkali metals like Li and K will also form cations with ______ charges.
 Why? ________________________
 Since other metals also have low ______________________________ they will also ____________ electrons and form _____________.
 Group 2 elements will lose ______ valance electrons and will end up with a ______ charge.
 Aluminum will lose 3 valance electrons and will end up with a _________ charge.
TRANSITION METALS AND GROUPS 3A AND 4A
 Tranistion metals and some of the group 3A and 4A elements don’t lose or gain enough electrons to have a completely ___________ octet.
 In fact many of the transition metals can form __________ than one ____________ ion.
 For example, Fe can lose two electrons to become _____ or it can lose three electrons to become ________

Name: __________________________________________________________ Date __________________________________ Period ___________
NAMING IONS
 When __________ like sodium become __________ they keep their names.
 When nonmetals like _________________ become
______________ their names change to have ___________at the end.
2 MORE THINGS
 When atoms become ions they no longer have the same
________________ as their _____________ atom.
 Also, ions usually take on the electron configuration of the nearest noble gas but they do not actually ________________ that noble gas.
 For example _____________ has the same electron configuration as Ne but it still has 11p+ so it doesn’t behave like _______.
FYI
You should be able to list the charges of the following ions just by looking at their location on the periodic table:
Alkali metals: H, Li, Na, K, Rb, Cs
Alkali Earth metals: Mg, Ca, Sr, Ba
Group 13: Al
Group 15: N, P
Group 16: O, S, Se
Group 17: F, Cl, Br, I