Shared Flashcard Set

Details

Chapter 5
Zeff,periodic table, mendeleev...
11
Chemistry
11th Grade
12/19/2007

Additional Chemistry Flashcards

 


 

Cards

Term

Explain:

 

Potassium has a lower first-ionization energy than lithium

Definition
As you go down the periodic table, n increases, potassium is larger than lithium and has less zeff than lithium and holds on to its valence e- less tightly. Therefore it is easier to remove valance e- from potassium, then it is from lithium.
Term

Explain: 

The ionic radius of N3-is larger than that of O2-

Definition

The more e- you gain, the larger the ion, and the lower the zeff. in addition e-/e- repulsions increase for both of these reasons nitrogen has less of a pull on its e- than O2-

 

N3-      O2-

   7:10    8:10    

 

 

Term

Explain:

A calcium atom is larger than a zinc atom

Definition

Zinc is greater than calcium becuase more protons are pulling on the same # of core e- which results in a smaller atom.

Term

Explain:

The second ionization energy of sodium is about three times greater than the second ionization energy of magnesium

 

Definition
It's harder to remove an e- from sodium because you would be taking from a core electron, whereas you wouldn't until the 3rd ionization energy level in Magnesium, zeff would be greater for sodium, and it's harder to remove core e- than valence e-.
Term
Why is helium a member of group 18 & not 2?
Definition
Because it is an inert gas and has a full valence shell.
Term
State 5 differences between metals and nonmetals
Definition

Metals:

luster, good conducters of heat and electricity, solid@ room temp., maleable, ductle 


Non Metals:

not luster, not good conducters of heat and electricity, gas a room temp, not maleable, not ductle

Term
relationship between group numbers & valence e- for main group elements
Definition

the valence e-= the 1's place

 

Ex: 13....valence e-=3

Term

How do modern day periodic tables differ from Mendeleev's?

(2 ways, must be in a chart)

Definition

Mendeleev:

increasing atomic mass, similar properties,by row


Modern:

increasing atomic #, elements w/similar properties, by groups(columns)

Term
Why is fluorine the most electrongative element?
Definition
As you go across the P.T. seff increases, but when you go down zeff decreases. Part of the halogens only holds one more e- to be stable. (has the greatest zeff, and is the smallest of the halogens) most likely to attract e- in a chemical bond.
Term
Why do halogens have the most negative electron?
Definition
Because they have the greatest zeff in each period, and are 1 electron away from being stable, which makes them the easiest elements to add an electron to.
Term
Which group has the lowest 1st ionization energies? WHY?
Definition
Group 1, because they have the lowest zeff and are the most to readily give up 1 e- to form stable ions.
Supporting users have an ad free experience!