Which one of the following species has a different number of electrons from all the others?
Cl-
Al3+
Ar
Ca2+
Which of the following elements has the lowest first ionisation energy?
K
Mg
Be
B
Which one of the following determines which element an atom will be?
Its number of protons
Its electric charge
Its number of neutrons
Its electron configuration
What is the maximum number of unpaired electrons possible in 3d orbitals?
5
10
3
6
Which statement best describes a covalent bond?
The atoms have formed an infinite network
The atoms have a noble gas electron configuration
There is simultaneous attraction of both nuclei to a shared electron pair
There is greater attraction of electrons to the more electronegative atom
Which one of the following statements is true?
H2O is polar, but H2S is non-polar
H2O has a greater molecular polarity (dipole moment) than H2S
The molecules H2S and H2O are both linear
The molecules H2S and H2O both have zero molecular polarity (dipole moment).
Which of the following has the highest first ionisation energy?
F
Mg
Si
S
An element Y has the electron configuration 1s22s22p5 and forms a compound XY2 with element X. Which one of the following could be the electron configuration of X?
1s22s2
1s22s22p1
1s22s22p2
1s22s22p63s1
Which of the following substances contains dispersion forces?
I CO2 II CH3CH2OH III SiO2
None of the given answers
I, II and III
I only
I and II only
Element A has the valence electron configuration of s2 and element B has the valence electron configuration of s2p5. What will be the most likely formula of the compound formed between the two elements?
A2B
AB
AB2
AB3
Species 'X' has the valence electron configuration of s2, and 'Z' has the valence electron configuration of s2p5. Which of the following is the most likely formula of a compound formed between 'X' and 'Z' ?
X2Z7
XZ2
X2Z5
XZ
How many orbitals can be found in the d subshell of the 3rd principal energy level?
8
3
5
10
Which one of the following lists the attractive forces in decreasing order (strongest to weakest)?
hydrogen bonding > van der Waals forces > covalent bonding