Periodic Law and Periodic Table
Chemistry ⇒ Atomic Structure and the Periodic Table
Periodic Law and Periodic Table starts at 8 and continues till grade 12.
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Describe the difference between a period and a group in the periodic table.
Describe the trend in metallic character as you move down a group in the periodic table.
Explain why elements in the same group have similar chemical properties.
Explain why noble gases are chemically inert.
Explain why the atomic radius decreases across a period from left to right.
Explain why the first ionization energy increases across a period.
State one reason why hydrogen is placed separately in the periodic table.
State the general trend of atomic size down a group.
Which of the following best describes the periodicity of properties?
(1) Random variation
(2) Repetition at regular intervals
(3) Decrease only
(4) Increase only
Which of the following elements has the largest atomic radius?
(1) Lithium
(2) Sodium
(3) Potassium
(4) Rubidium
Which of the following elements is a metalloid?
(1) Silicon
(2) Sodium
(3) Oxygen
(4) Iron
Which of the following elements is a transition metal?
(1) Sodium
(2) Iron
(3) Calcium
(4) Sulfur
The atomic number of an element is equal to the number of _______ in its nucleus.
The d-block elements are also known as _______.
The element with atomic number 20 is classified as a _______.
The element with atomic number 26 is called _______.
True or False: Elements in the same group have similar chemical properties.
True or False: Elements in the same period have the same number of valence electrons.
True or False: The lanthanides and actinides are placed separately at the bottom of the periodic table to keep the table more compact.
True or False: The periodic table can be used to predict the chemical behavior of elements.
