Trends
Trends
Trends
Bonds
Misc.
100
What is the trend in metallic character as you move from left to right across the periodic table?
Metallic character decreases.
100
What is the trend in ionic size as you move from left to right across the periodic table?
Overall ionic size decreases from left to right.
100
List the following elements in order of increasing atomic radius: Na, Cl, S, K
Cl < S < Na < K
100
Why do elements bond?
To become stable, have a full valence shell, obtain an octet, attain a noble gas like configuration.
100
List the following elements in order of increasing ionic size: Na+; Mg2+; Al3+
Al3+ < Mg2+ < Na+
200
Which group of elements is more reactive, alkali metals or alkaline earth metals?
Alkali metals.
200
What is the effective nuclear charge felt by the valence electrons in an atom of Magnesium?
+2; same as the grou number or number of valence electrons.
200
List the following elements in order of increasing ionization energy: Cs, Ca, K, Be
Cs < K < Ca < Be
200
A difference in electronegativity greater than or equal to 1.8 indicates what type of bond?
An ionic bond.
200
What happens to effective nuclear charge as you move down a group?
It stays the same.
300
State the relationship between the size of a cation and an anion to the neutral atom they have formed from.
A cation is smaller (lost electrons) and an anion is larger (gained electrons)
300
State the trend in reactivity as you move from top to bottom in groups 1 and 2 on the periodic table and explain why it occurs.
Reactivity increases as you move from top to bottom because it is easier to remove an electron from an atom that has more shielding of the nuclear charge than from one with less shielding.
300
List the following elements in order of increasing electronegativity: C, Mg, Si, Ca
Ca < Mg < Si < C
300
What type of bond would form between calcium and iodine?
Polar covalent.
300
Provide an example of a metal and a nonmetal that would form a covalent bond.
Any two elements whose difference in electronegativity would be less than 1.8.
400
State the trend in atomic size/radius as you move from top to bottom on the periodic table and explain why this occurs.
The atomic size/radius increases from top to bottom because the number of occupied energy levels within the atom is increasing.
400
State the trend in ionization energy as you move from top to bottom on the periodic table and explain why this occurs.
Ionization energy decreases as you move from top to bottom because as you add energy levels you increase the degree of shielding of the nuclear charge which means the pull from the nucleus is reduced so the valence electrons are held onto less tightly and less energy is needed to remove them.
400
State the trend in electronegativity as you move from top to bottom on the periodic table and explain why this occurs.
Electronegativity decreases as you move from top to bottom because the number of energy levels is increasing, therefore the amount of shielding increases which means neighboring electrons can't get close to or feel much of the charge emanating form the nucleus.
400
Which bond would be most polar: C - H or S - O?
S - O
400
Which element in a bond between P and Cl would be labeled as partially positive and which would be partially negative?
P = partial positive; Cl = partial negative
500
State the trend in atomic radius/size as you move from left to right across the periodic table and explain why this trend occurs.
Atomic size/radius decreases as you move from left to right because the overall nuclear charge and the effective nuclear charge increases, pulling the electrons in closer to the nucleus.
500
State the trend in ionization energy as you move from left to right across the periodic table and explain why this trend occurs.
Ionization energy increases as you move from left to right because the nuclear charge is increasing and therefore the nucleus has a stronger pull on his eletcrons, and hangs on to them more tightly, requiring more energy for removal.
500
State the trend in electronegativity as you move from left to right across the periodic table and explain why this trend occurs.
Electronegativity increases as you move from left to right because the nuclear charge is increasing meaning the strength of pull from the nucleus is increasing and the size of the atom is decreasing, therefore neighboring electrons can get closer to and feel much more attracted to the nucleus of the elements towards the right of the periodic table.
500
Provide a description of a metallic bonding.
Positive metal ions in a sea of delocalized electrons.
500
Explain why metals are malleable, ductile and can conduct electricity.
Because they have Freely Moving Charged Particles, that can slide past each other making them flexible and also allowing current to transfer through them.
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