Electronegativity
Atomic Radius
Naming Ionic Compounds
Ionization Energy
Groups in the Periodic Table
100
True or false? Electronegativity is a number that describes the relative ability of an atom, when bonded, to attract electrons. The when it trends down on the period table, it increases.
False
100
Fill in the blank. Atomic radius is defined as ________ from the outermost orbital to the nucleus
Distance
100

Whis is bigger Ca or O-2

O-2

100
Which element has higher ionization energy? Carbon or aluminum
Carbon
100
Hydrogens, carbon , nitrogen are all examples of...?
non-metals
200
What is electronegativity used for?
Electronegativity is used to see if a bond is either polar or covalent
200
when atomic radius trends down a group why does it increase?
More orbitals; less attraction between the valence electrons and protons in nucleus.
200

Which has a larger ionization energy Mg or N?

N

200
Which element has higher ionization energy? Sulfer or Chlorine
Chlorine
200
Boron silicon are examples of____?
metalloids
300
using their location on the periodic table, determine the rank from least to greatest with the elements: Cl, Mg,Ca,N, and O
Ca,Mg,N,Cl and O
300
Define atomic radius
Is a measure of the size of its atom or the distance from the valence shell to the atom its self
300

Which has a larger nuclear charge Fe or S? why?

Fe

300
Does the trend for ionization energy across the periodic table increase or decrease? and why?
Increase - smaller radius, electron is closer to the nucleus which makes it more difficult to pull
300
Which trends in the periodic table increase across and decrease downwards?
electron affinity, electronegativity, ionization energy
400
Predict which of the following elements has the largest En and state why? Na and Rb
sodium is higher because sodium is higher then Rb in the periodic table.
400
When atomic radius trends across does it increase or decrease and why?
Decreases - has the same # of orbitals, more protons and elections therefore greater attraction and pull towards the nucleus
400

Which will experience a stronger effective nuclear charge, an outermost electron in Fe or S? and why?

S

400
Define Ionization energy?
the energy required to remove a valence electron from an atom in its gaseous state.
400
Which trends in the periodic table increase downwards and decrease across?
Atomic radius, reactivity
500
How does the trend go for Electronegativity and explain why
Trend down - the larger atom will pull less strongly on the electron pair since they are further to its nucleus Trend across - the smallest atom will pull more strongly on the election pair since they are closer to its nucleus
500
Using their location on the periodic table, rank the size of follwoing sets of elements in order of increasing atomic size. Mg, S, Cl,Li, Cs and K
Cl, S, Mg, K, Cs
500

arrange in order of increasing electronegativity:

Cs, He, Ca, F


Cs, Ca,F, He

500
In an ionization energy, when the trend goes down, what happens? and why?
the trend decrease - more orbitals, electron further from nucleus and it is easier to remove an electron
500
Who invented the periodic table
Dmitri Mendeleev
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