So trendy
This trend in the periodic table increase as you go down a group and decrease as you move from left to right across the periodic table
Atomic radius
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.
The energy required to remove an electron from atom.
What is ionization energy?
The ion form of Hydrogen
H+
Hydrogens, carbon, neon are all examples of...?
non-metals
I determine the name and type of atom
Protons / Atomic Number
I am the most reactive non-metal. I am also the most electronegative element.
Fluorine
These 2 trends increase as you go from left to right across the periodic table and decrease as you go down a group.
Electronegativity and ionization energy
Which element has higher ionization energy? Carbon or aluminum
Carbon
Distance from the outermost orbital to the nucleus
Atomic radius
The element that loses an electron easier than any other atom.
francium (Fr)
The class that germanium, boron, and silicon belongs to
metalloids
I am an alkali earth metal with 3 energy levels.
Magnesium / Mg
This is why alkali metals are more reactive than alkaline earth metals
Alkali metals are more reactive because they more easily lose an electron compared to alkaline earth metals.
This explains why the atomic radius increases as you move down the periodic table
More electron shells add more distance between the nucleus and the valence electron shell (outer most electrons)
DAILY DOUBLE
Arrange the following in order of increasing ionic radius:
Br ion, At ion, Cl ion, F ion
F ion < Cl ion < Br ion < I ion
(All are halogens; charge is -1)
The reason that Na has a smaller electronegativity than Rb.
Sodium is higher in the group than Rb, so the size will decrease. A smaller atomic radius means more pull on the electrons by the nucleus, keeping them closer to the atom.
The charge of the chlorine ion
(Answer must include + or - and number; sign and magnitude)
Cl-1
These elements have similar properties to Rb
Li, Na, K, Ca, Fr
Accept: Alkali metals
Do not accept: hydrogen unless stated that it has similar reactivity due to 1 valence electron but does not have similar physical properties.
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.
Calculate Zeff for an atom of sulfur
Zeff = Z - S
Z = # of protons
S = # of core electrons
Zeff = +6
DAILY DOUBLE
This explains why the atomic radius decreases as you move from left to right across a period.
Electrons are closer to the nucleus which makes it more difficult to pull
Greater effective nuclear charge makes it more difficult to lose an electron
more protons but same number of core electrons therefore greater attraction and pull towards the nucleus
The ranking order of the following elements by increasing atomic size
Mg, S, Cl, Li, Cs and K
Li, Cl, S, Mg, K, Cs
The reason these main group elements will have an increased atomic radius when they become ions.
(Answer must include the 3 groups of elements & the reasoning for the increased size for the ions)
Groups 5, 6, 7 - form anions (gain electrons)
Effective nuclear charge is not as powerful as these elements gain an electron, so the electrons repel each other more. This causes an increase in the radius.
Anions have this type of charge
Negative
The number of valence electrons present in group 15 atoms
5
The most electronegative element
What is Fluorine?
Explanation: Fluorine has the greatest effective nuclear charge.
In group 2, which element is the most reactive?
Ra
This explains why the electronegativity decreases as you move from left to right across the periodic table.
Smallest atom will pull more strongly on the electron pair since they are closer to its nucleus
Which element has higher ionization energy? Sulfur or Chlorine
Chlorine
This is the opposite of process as ionization energy; it is the energy change that happens when an atom gains an electron. Surprisingly, the trend is the same as the ionization energy trend.
Electron affinity
Metals will always do this to form a charge. The charge is always this sign.
Lose electrons.
Cations / positive
These are 2 properties of metals
solid at room temp
shiny appearance (luster)
conduct electricity
are malleable and ductile
I am not a metal nor a non-metal and have 5 valence electrons. This is my name and my elemental class
Antimony / Sb OR Arsenic / As
Metalloid
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.