Electronegativity decreases down a group because

extra energy level and shielding

Shielding increases with....

an increasing number of inner electrons

The covalent radius of an elements is described as....

half the distance between the nuclei of two bonded atoms

Why is the 2nd ionisation energy of sodium much larger than the first?

an electron is being removed from a stable shell closer to nucleus

ionisation energy is the amount of energy required to

remove one mol of electrons from one mole of gaseous atoms

Going down a group covalent radius increases because

shielding and extra energy shell

In The Periodic table, going across a period the covalent radius decreases due to the .....

increased positive charge on the nucleus

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Periodicity - Higher Chemistry

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Trends in The Periodic table

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Questions 20

Answers

1
Electronegativity decreases down a group because
extra energy level and shielding
decreasing nuclear charge
one less energy level and shielding
increasing nuclear charge
2
Which element is the most electronegative?
Nitrogen
Helium
Calcium
Fluorine
3
Elements are arranged in the periodic table in order of
decreasing size
increasing size
increasing atomic number
decreasing atomic number
4
Across a period...
electronegativity decreases
covalent radius increases
ionisation energy increases
atomic size increases
5
Shielding increases with....
increased nuclear charge
an increasing number of inner electrons
decreased nuclear charge
a decreasing number of energy levels
6
The covalent radius of an elements is described as....
half the distance between the electrons of two bonded atoms
half the distance between the nuclei of two bonded atoms
double the distance between the nuclei of two bonded atoms
half the distance between the electrons and the nucleus
7
Why is the 2nd ionisation energy of sodium much larger than the first?
an electron is being removed from a stable shell closer to nucleus
an electron is removed from a stable shell further away from nucleus
covalent radius is larger
an electron is being added to a stable shell
8
the first ionisation energy of bromine is...
Br(g) → Br +(g) + e-
Br+(g) → Br 2+(g) + 2e-
Br2(g) → Br +(g) + e-
Br(g) → Br 2+(g) + 2e-
9
ionisation energy is the amount of energy required to
remove an electron from one mole of gaseous atoms
add one mol of electrons from one mole of gaseous atoms
remove one mol of electrons from one mole of gaseous atoms
add an electron to one mole of gaseous atoms
10
Going down a group covalent radius increases because
shielding only
increasing nuclear charge and extra energy shell
increasing nuclear charge only
shielding and extra energy shell
11
Periodicity is the occurrence of what in the Periodic table?
rows
groups
patterns
metals and non-metals
12
What is a measure of the attraction an atom has for bonding electrons?
ionisation energy
electronegativity
covalent radius
atomic size
13
Down a group
atomic size increases
ionisation energy increases
electronegativity increases
covalent radius decreases
14
The bigger the covalent radius
the smaller the atom
the bigger the ionisation energy
the smaller the atomic number
the larger the atom
15
In The Periodic table, going across a period the covalent radius decreases due to the .....
decreased positive charge on the nucleus
increase in the number of energy levels
increased positive charge on the atom
increased positive charge on the nucleus
16
Which of the following has the least attraction for bonding electrons?
phosphorus
carbon
nitrogen
silicon
17
What is the trend in covalent radius going down a group
Increasing
increases then decreases
Decreasing
Stays the same
18
The following equation represents what ionisation energy: Li⁺(g) → Li²⁺(g) + e^-
3rd
1st
2nd
4th
19
What happens to electronegativity as you go across a period?
goes up and then down
increases
stays the same
decreases
20
Going down a group in The Periodic table the size of the atom...
increases
does not change
decreases
goes up and then down

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