EduNinja
[Maximum number: 1]

Which pair of formulae is correct?

A

Ag2CO3\mathrm{Ag}_{2} \mathrm{CO}_{3} and (NH4)3NO3\left(\mathrm{NH}_{4}\right)_{3} \mathrm{NO}_{3}

B

K2HCO3\mathrm{K}_{2} \mathrm{HCO}_{3} and Zn3(PO4)2\mathrm{Zn}_{3}\left(\mathrm{PO}_{4}\right)_{2}

C

AgHCO3\mathrm{AgHCO}_{3} and K3PO4\mathrm{K}_{3} \mathrm{PO}_{4}

D

ZnCO3\mathrm{ZnCO}_{3} and (NH4)2PO4\left(\mathrm{NH}_{4}\right)_{2} \mathrm{PO}_{4}

[Maximum number: 1]

Which atom has exactly three unpaired electrons in the ground state?

A

an isolated gaseous aluminium atom

B

an isolated gaseous carbon atom

C

an isolated gaseous chromium atom

D

an isolated gaseous phosphorus atom

[Maximum number: 1]

Which atom has its outermost electron in an orbital of the shape shown, with principal quantum number 3 ?

Question image
A

sodium

B

chlorine

C

calcium

D

bromine

[Maximum number: 1]

A simple ion X+X^{+}contains eight protons.
What is the electronic configuration of X+\mathrm{X}^{+}?

A

1s22s12p61 s^{2} \quad 2 s^{1} \quad 2 p^{6}

B

1s22s22p3\begin{array}{rrr}1 s^{2} & 2 s^{2} & 2 p^{3}\end{array}

C

1s22s22p51 s^{2} \quad 2 s^{2} \quad 2 p^{5}

D

1s22s22p7\begin{array}{rrr}1 s^{2} & 2 s^{2} & 2 p^{7}\end{array}

[Maximum number: 3]

The elements phosphorus, sulfur and chlorine are in Period 3 of the Periodic Table.

Table 1.1 shows some properties of the elements P to Cl .
The first ionisation energy of S is not shown.

Table 1.1

Table 1.1

(a)
(i)

Complete Table 1.1 to show the number of electrons in the 3 p subshell and the total number of unpaired electrons in an atom of P, S and C 1 .

[ 2 ]
(b)

P3−,S2−\mathrm{P}^{3-}, \mathrm{S}^{2-} and Cl−\mathrm{Cl}^{-}have the same number of electrons.

[ 1 ]
(i)

Give the full electronic configuration of P3−\mathrm{P}^{3-}.

[ 1 ]
[Maximum number: 2]

The elements silicon, phosphorus and sulfur are in Period 3 of the Periodic Table.

(a)

Table 1.1 shows some properties of the elements Si to S .

The first ionisation energy of P is not shown.

Table 1.1

Table 1.1

[ 2 ]
(i)

Complete Table 1.1 to show the total number of s and p electrons in an atom of Si, P and S .

[ 2 ]
[Maximum number: 1]

Copper is used in electrical equipment. It has a melting point of 1085∘C1085^{\circ} \mathrm{C}.

(a)

When KI(aq) is added to CuSO4(aq)\mathrm{CuSO}_{4}(\mathrm{aq}) the blue-coloured solution turns brown and a white precipitate of CuI(s) is seen.

The reaction between copper ions and iodide forms only two products.

[ 1 ]
(i)

State the full electronic configuration of Cu2+\mathrm{Cu}^{2+}.

[ 1 ]
[Maximum number: 4]

Tellurium is an element in Group 16. The most common isotope of tellurium is 130Te{ }^{130} \mathrm{Te}. Its electronic configuration is [Kr]4 d105 s25p4[\mathrm{Kr}] 4 \mathrm{~d}^{10} 5 \mathrm{~s}^{2} 5 p^{4}.

(a)

Complete Table 1.1.

Table 1.1

Table 1.1

[ 3 ]
(b)

Identify the sub-shell in an atom of Te that contains electrons with the lowest energy.

[ 1 ]
[Maximum number: 1]

The Pauling electronegativity values of elements can be used to predict the chemical properties of compounds.

Use the information in Table 1.1 to answer the following questions.

Table 1.1

Table 1.1

(a)
(i)

Give the full electronic configuration of S2+(g)\mathrm{S}^{2+}(\mathrm{g}).

[ 1 ]
[Maximum number: 1]

Atoms with nuclei containing an odd number of protons tend to have fewer isotopes than those with an even number of protons.

(a)

Potassium also has two stable isotopes. Both isotopes have the same chemical properties.

[ 1 ]
(i)

State the full electronic configuration of an atom of potassium.

[ 1 ]
0