Electronegativity
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
Fill in the blank. Atomic radius is defined as ________ from the outermost orbital to the nucleus
Distance
Which element has higher ionization energy? Carbon or aluminum
Carbon
Hydrogens, carbon , nitrogen are all examples of...?
non-metals
What is electronegativity used for?
Electronegativity is used to see if a bond is either polar or covalent
When atomic radius trends down a group why does it increase?
More orbitals; less attraction between the valence electrons and protons in nucleus.
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 electronegativity from least to greatest with the elements: F, Mg,Ca,N, and O
Ca,Mg,N,O and F
Define atomic radius
Is a measure of the distance from the valence shell to the atom its self
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 off an electron
Which two trends in the periodic table increase across and decrease downwards?
electronegativity and ionization energy
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 the periodic table.
When atomic radius trends across the periodic table, 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
Define Ionization energy?
the energy required to remove a valence electron from an atom in its gaseous state.
Which trend in the periodic table increases downwards and decreases across?
Atomic radius
How does the trend go (across and down) 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 follwoing sets of elements in order of increasing atomic size. Mg, S, Cl, F, Cs and K
F, Cl, S, Mg, K, Cs
In an ionization energy,how does the trend go down a group? Why?
the trend decreases - more orbitals, electron further from nucleus and it is easier to remove an electron
Who if the "Father" of the periodic table
Dmitri Mendeleev