Classification of Elements and Periodicity in Properties
Test 6

Correct answer Carries: 4.

Wrong Answer Carries: -1.

What is the formula of the compound formed between phosphorus and oxygen in its highest oxidation state?

P (group 15, valence 5 in +5 state) forms \(\ce{P2O5}\) with oxygen (valence 2), a stable acidic oxide.

\(\ce{PO}\)
\(\ce{PO2}\)
\(\ce{P2O5}\)
\(\ce{P2O3}\)
3

What is the temporary systematic name of the element with atomic number 113?

For \(Z=113\): 1 (un), 1 (un), 3 (tri) → ununtrium (before being named Nihonium).

Ununpentium
Ununseptium
Ununoctium
Ununtrium
4

Which of the following nitrates decomposes most readily to form a basic oxide?

Group 2 nitrates decompose to basic oxides, \(\ce{NO2}\), and \(\ce{O2}\). \(\ce{Be(NO3)2}\) decomposes most readily to \(\ce{BeO}\) (basic) due to Be²⁺’s small size and high charge density, which weakens the nitrate lattice.

A. \(\ce{Mg(NO3)2}\)
B. \(\ce{Be(NO3)2}\)
C. \(\ce{Ca(NO3)2}\)
D. \(\ce{Sr(NO3)2}\)
2

What is the formula of the compound formed between aluminium and sulfur?

Al (group 13, valence 3) and S (group 16, valence 2) form \(\ce{Al2S3}\) by cross-multiplying valences, a stable ionic compound.

\(\ce{AlS}\)
\(\ce{AlS2}\)
\(\ce{Al2S3}\)
\(\ce{Al3S2}\)
3

What is the formula of the compound formed between boron and fluorine?

B (group 13, valence 3) and F (group 17, valence 1) form \(\ce{BF3}\), a stable covalent compound, unlike \(\ce{BF}\), \(\ce{BF2}\), or \(\ce{B2F3}\).

\(\ce{BF}\)
\(\ce{BF2}\)
\(\ce{BF3}\)
\(\ce{B2F3}\)
3

Which element in group 13 has the lowest third ionization enthalpy?

Third ionization enthalpy decreases down group 13 as size increases, reducing nuclear attraction. Tl (period 6) has the lowest value among B, Al, Ga, and Tl.

B
Al
Ga
Tl
4

What is the formula of the compound formed between germanium and oxygen?

Ge (group 14, valence 4) forms \(\ce{GeO2}\) with oxygen (valence 2), a stable covalent oxide, unlike \(\ce{GeO}\), \(\ce{Ge2O}\), or \(\ce{GeO4}\).

\(\ce{GeO}\)
\(\ce{Ge2O}\)
\(\ce{GeO2}\)
\(\ce{GeO4}\)
3

Which element in group 17 has the lowest electron affinity?

Electron affinity decreases down group 17 due to increasing size and reduced nuclear attraction. I (period 5) has the lowest value among F, Cl, Br, and I.

F
Cl
Br
I
4

Which of the following has the smallest ionic radius?

For isoelectronic species (\(\ce{O^2-}\), \(\ce{F^-}\), \(\ce{Na+}\), \(\ce{Mg^2+}\), all with 10 electrons), radius decreases with increasing nuclear charge. \(\ce{Mg^2+}\) (Z=12) has the smallest radius.

\(\ce{O^2-}\)
\(\ce{Mg^2+}\)
\(\ce{F^-}\)
\(\ce{Na+}\)
2

Which element has the ground state electronic configuration \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^6 4s^2\)?

This configuration (Z=26) corresponds to Fe (period 4, group 8), with \(3d^6 4s^2\), distinguishing it from Mn (\(3d^5 4s^2\)), Co (\(3d^7 4s^2\)), or Ni (\(3d^8 4s^2\)).

Mn
Fe
Co
Ni
2

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