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Worksheets4. Basic Chemistry: Periodic Table
Total questions: 25
Worksheet time: 25mins
How is this relationship showed in the properties of the elements in the same group?
They have different electron configurations
They have similar chemical properties
They have different number of orbitals
What group in periodic table would have five valence electrons?
Group 1A
Group 5A
Group 7B
Group 2B
Group 3A
What types of ions do the metals and the non-metallic elements form?
Metals and non-metallic elements do not form ions
Metals form positive ions and non-metallic elements form negative ions
Give some similarities that exist among the elements of Group 7A.
All exist as diatomic molecules
They all are non-metals
They have relatively high electronegativities and form -1 ions in reacting with metallic elements
Which of the following elements most easily gives up electrons during reactions?
Potassium
Chloride
In the following sets of elements, indicate which element has the smallest atomic size. Ba, Ca, P, Si, Al.
Al
Metals have relatively ........... ionization energies, whereas non-metals have relatively ........... ionization energies.
low, none
high, none
What name is given to the series of ten elements in which the electrons are filling the 3d sublevel?
Halogen
Transition Metals
What are the metalloids?
Gold, Silver, Copper, Iron.
Boron, Silicon, Germanium, Arsenic.
Hydrogen, Helium, Lithium, Beryllium.
Oxygen, Carbon, Nitrogen, Fluorine.
Lithium, Sodium, Potassium, Magnessium.
Rows on the period table are called .................... while columns are called .......................
groups, families
groups, periods
Which of the following groups is non-metallic and has the outermost electron configuration of the form ns2np5?
Chemical elements in the same group A have the following properties
As the nuclear charge increases, the metallic character increases, and the non-metallic character increases.
As the nuclear charge increases, the metallic character increases and the non-metallic character decreases.
As the nuclear charge decreases, the metallic character increases and the non-metallic character decreases.
As the nuclear charge decreases, the metallic character decreases and the non-metallic character decreases.
No correct answer.
Which elements are not in the same group?
Li, Na, K
Ca, Sr, Ba
Be, Mg, Cr
Ge, Sn, Bi
Cl, Br, I
Element ‘X’ forms a chloride with the formula XCl2, which is a solid with high melting point. X would most likely be in the same group of the periodic table as ................
Al
Ca
F
C
A groups elements react similarly because of their .........
number of neutron
valence electrons
Which of the following statements is/are not correct about the trends in the properties of the elements of a period on going from left to right?
the metallic character increase
the ionization energy increase
Atoms of which of the following groups of elements do not tend to donate or accept electrons?
Which one of the following statements is/are correct about the trends of effective nuclear charge?
As we move from left to right on the periodic table, effective nuclear charge increase.
As we move from top to bottom the periodic table, effective nuclear charge decrease.
As we move from left to right on the periodic table, effective nuclear charge decrease.
As we move from top to bottom the periodic table, effective nuclear charge increase.
The size of ionic Na+ > Mg2+ > Al3+. Which of the followings explain(s) this trend?
The number of proton is the same but the number of electron is decrease.
Atomic number decrease.
Electron affinity increase.
Effective nuclear charge increase.
Ionization energy decrease.
Going down a group in the periodic table ...................
the metallic characters increase
the electron affinity increase
the atomic size increases
the ionic size increase
the ionization energy increase
Which of the following values will increase as you move from left to right on the Periodic Table?
Ionic radius
Atomic radius
Effective nuclear charge
Element P, Q and R have 18, 19 and 20 protons respectively. It is found that the atomic size of P is the smallest. What is the factor that influences its size?
Least number of shells
Largest effective nuclear charge
Smallest relative atomic mass
The higher the ionization energy ...
the less attracted the valence electron is to the nucleus
the less attracted the valence electron is to another electron
Electronegativity .................. from left to right within a period and .................. from top to bottom within a group.
What is the tendency of an atom to attract electrons towards itself?
Atomic radius
Electron affinity
Ionization energy
Nuclear charge
