Electronegativity
True or false? Electronegativity decreases as you go down a group.
False
Fill in the blank. Atomic radius is defined as ________ from the outermost orbital to the nucleus
Distance
The vast majority of elements are metals, nonmetals or metalloids.
metals
Which element has higher ionization energy? Carbon or aluminum
Carbon
Hydrogens, carbon , nitrogen and helium are all examples of...?
non-metals
Which of these would have the greatest electronegativity? Na, Ca, F, Mg
Fluorine, it is a nonmetal
As you go down a group, why does atomic radius increase increase?
More orbitals; less attraction between the valence electrons and protons in nucleus.
All members of the same group have the same number of ______________. All members of the same period have the same number of _______________.
valence electrons, energy levels
Which element has higher ionization energy? Sulfur or Chlorine
Chlorine
Boron silicon are examples of____?
metalloids
using their location on the periodic table, determine the rank from least to greatest with the elements: F, Mg,Ca, N, and O
Ca, Mg, N, O, F
Define atomic radius
Is a measure of the size of its atom or the distance from the valence shell to the atom its self
Which trends in the periodic table increase across and decrease downwards?
electronegativity, ionization energy
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
Noble Gases
Predict which of the following elements has the largest electronegativity and state why? Na and Rb
sodium is higher because sodium is higher then Rb in their group, meaning its radius is smaller
As you head from left to right on a period, what happens to atomic radius and why?
Decreases - has the same # of orbitals, more protons therefore greater attraction and pull towards the nucleus
Which two trends in the periodic table increase downwards and decrease across?
Atomic radius, ionic radius
Define Ionization energy?
the energy required to remove a valence electron from an atom in its gaseous state.
What are the group 17 elements called?
Halogens
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
Using their location on the periodic table, rank the size of following sets of elements in order of increasing atomic size. Mg, S, Cl, Li, Cs and K
Cl, S, Mg, K, Cs
Mg forms an ion. Compare its ionic radius to its atomic radius and explain why this difference exists.
Ionic radius is smaller because all the valence electrons are lost and, therefore, one less orbital is occupied.
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
These two rows of elements are separated from the periodic table so that it will line up correctly and not be too wide.
Lanthanoids and Actanoids