Electronegativity
True or false? Electronegativity is a number that describes the relative ability of an atom, when bonded, to attract electrons. Going down a group on the periodic table, the electronegativity 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
The ion form of Hydrogen
H+
Hydrogens, carbon , nitrogen are all examples of...?
non-metals
I determine what type of atom I am.
Protons / Atomic Number
Properties of Metals
solid at room temp
shiny appearance (luster)
conduct electricity
are malleable and ductile
The most electronegative element
What is Fluorine?
Explanation: Fluorine has the greatest effective nuclear charge.
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? Sulfer or Chlorine
Chlorine
How many valence electrons do elements in group 15 have and what kind of ion will they typically form?
5, anions
Boron and silicon are examples of____?
metalloids
The ion form of Cl
Cl-1
Compare the reactivity of an alkali metal to an alkaline earth metal
Alkali metals are more reactive because they more easily lose an electron compared to alkaline earth metals.
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
The element in period 5 with the largest atomic radius.
Rubidium (Rb)
Explanation: Rubidium is in group 1, it has the weakest effective nuclear charge of the elements in period 5.
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
Why does it take more energy to remove the second electron from an ion than it did the first?
The effective charge of the nucleus increases, holding remaining electrons more tightly
Which trends in the periodic table increase across and decrease downwards?
electron affinity, electronegativity, ionization energy
I am an alkali earth metal with 3 energy levels.
Magnesium / Mg
Calculate Zeff for an atom of sulfur
Zeff=+6
Zeff=Z(protons)-S(shielding electrons)
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.
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
DAILY DOUBLE
The energy required to remove a second electron, after one has already been removed.
What is second ionization energy?
Explanation: ionization energy is the energy to remove an electron, if one has already been previously removed, we are now looking at the second ionization energy aka the energy to remove a second electron.
Where are the two most reactive elements on the periodic table?
Top of the Halogens and Bottom of the Alkali metals
Which trends in the periodic table increase downwards and decrease across?
Atomic radius, reactivity
I am the most reactive non-metal.
Fluorine
Of the trends we discussed, which is not a very clear trend on the PT?
electron affinity
How do the trends 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
Li, Cl, S, Mg, K, Cs
The element in the pair with the higher first Ionization energy:
N or Si
What is Nitrogen (N)?
Explanation: Nitrogen is both above and to the right of Silicon. Ionization energy increases up and to the right on the table.
In general, as you go across a period in the periodic table from left to right: the atomic radius ________; the electronegativity _________; and the first ionization energy ________.
decreases, increases, increases
In group 2, which element is the most reactive?
Ra
I am not a metal nor non-metal and have 5 valence electrons
Antimony / Sb
Arsenic / As
Which main groups of elements will have a larger atomic radius when they become ions? Why?
Groups 5, 6, 7
because they become anions and the effective nuclear charge goes down as they gain an electron so their radius becomes larger.
Explain Coulomb's law. Which 2 factors does Coulomb's law depend on?
Coulomb's law states that the force between two atoms depends upon the distance between them and the size of the charge.
The larger the distance, the smaller the force.
The larger the size of the charge, the greater the force between them.