Classification of Elements and Periodicity in Properties

Metallic character generally:

1. Increases from left to right in a period
2. Decreases down a group
3. Decreases from left to right in a period
4. Remains constant

Which element belongs to the p-block?

1. Sodium
2. Magnesium
3. Chlorine
4. Calcium

The tendency of an atom to attract electrons towards itself in a compound is called:

1. Ionisation energy
2. Electron affinity
3. Electronegativity
4. Atomic radius

Which of the following has the highest ionisation energy?

1. Sodium
2. Magnesium
3. Aluminium
4. Neon

The block to which an element belongs depends on:

1. Atomic mass
2. Number of neutrons
3. Last electron entering orbital
4. Number of isotopes

The modern periodic law states that the properties of elements are periodic functions of:

1. Atomic mass
2. Atomic number
3. Density
4. Atomic volume

The elements placed in Group 18 are called:

1. Alkali metals
2. Halogens
3. Noble gases
4. Transition elements

The element with the largest atomic size in Period 3 is:

1. Sodium
2. Magnesium
3. Chlorine
4. Silicon

The first ionisation energy generally:

1. Decreases across a period
2. Increases across a period
3. Remains constant
4. Becomes zero

The most reactive metals are found in:

1. Group 1
2. Group 17
3. Group 18
4. Group 14

Atomic radius generally decreases across a period because:

1. Number of shells decreases
2. Nuclear charge increases
3. Electrons are removed
4. Atomic mass decreases

The element with the highest electronegativity is:

1. Oxygen
2. Nitrogen
3. Fluorine
4. Chlorine

Elements in the same group of the periodic table have similar:

1. Atomic masses
2. Number of shells
3. Valence electron configurations
4. Atomic sizes

The number of periods in the modern periodic table is:

1. 5
2. 6
3. 7
4. 8

The modern periodic table is arranged on the basis of:

1. Atomic mass
2. Atomic number
3. Number of neutrons
4. Atomic volume