Phosphorus forms a compound with hydrogen called phosphine, $$$\mathrm{PH}_{3}$$$. This compound can react with a hydrogen ion, $$$\mathrm{H}^{+}$$$. Which type of interaction occurs between $$$\mathrm{PH}_{3}$$$ and $$$\mathrm{H}^{+}$$$?

dative covalent bond

dipole-dipole forces

hydrogen bond

ionic bond

Chemistry

IGCSE&ALevel

CAIE

Exam No：9701_w24_qp_11 Year：2024 Question No：5

Answer:

Knowledge points:

3.4.1.1.1 hydrogen,

3.4.1.1.10 ethene,

3.4.1.1.2 oxygen,

3.4.1.1.3 nitrogen,

3.4.1.1.4 chlorine

3.4.1.1.5 hydrogen chloride, HCl

3.4.1.1.6 carbon dioxide,

3.4.1.1.7 ammonia,

3.4.1.1.8 methane,

3.4.1.1.9 ethane,

3.4.1.2 understand that elements in period 3 can expand their octet including in the compounds sulfur dioxide, , phosphorus pentachloride, , and sulfur hexafluoride,

3.4.1.3 describe coordinate (dative covalent) bonding, including in the reaction between ammonia and hydrogen chloride gases to form the ammonium ion, , and in the molecule

3.4.2.1.1 $\sigma $ bonds are formed by direct overlap of orbitals between the bonding atoms

3.4.2.1.2 π bonds are formed by the sideways overlap of adjacent p orbitals above and below the σ bond

3.4.2.2 describe how the σ and π bonds form in molecules including

3.4.2.3 use the concept of hybridisation to describe sp, $\mathrm{sp}^{2}$ and $\mathrm{sp}^{3}$ orbitals

3.4.3.1.1 bond energy as the energy required to break one mole of a particular covalent bond in the gaseous state

3.4.3.1.2 bond length as the internuclear distance of two covalently bonded atoms

3.4.3.2 use bond energy values and the concept of bond length to compare the reactivity of covalent molecules

7.2.1 state the names and formulae of the common acids, limited to hydrochloric acid, HC/, sulfuric acid, ethanoic acid,

7.2.10 select suitable indicators for acid-alkali titrations, given appropriate data

7.2.2 state the names and formulae of the common alkalis, limited to sodium hydroxide, NaOH, potassium hydroxide, KOH, ammonia,

7.2.3 describe the Brønsted–Lowry theory of acids and bases

7.2.4 describe strong acids and strong bases as fully dissociated in aqueous solution and weak acids and weak bases as partially dissociated in aqueous solution

7.2.5 appreciate that water has pH of 7, acid solutions pH of below 7 and alkaline solutions pH of above 7

7.2.6 explain qualitatively the differences in behaviour between strong and weak acids including the reaction with a reactive metal and difference in pH values by use of a pH meter, universal indicator or conductivity

7.2.7 understand that neutralisation reactions occur when

7.2.8 understand that salts are formed in neutralisation reactions

7.2.9 sketch the pH titration curves of titrations using combinations of strong and weak acids with strong and weak alkalis

Phosphorus forms a compound with hydrogen called phosphine, $$\(\mathrm{PH}_{3}\)$$. This compound can react with a hydrogen ion, $$\(\mathrm{H}^{+}\)$$. Which type of interaction occurs between $$\(\mathrm{PH}_{3}\)$$ and $$\(\mathrm{H}^{+}\)$$?

Answer:

Knowledge points:

Solution:

Phosphorus forms a compound with hydrogen called phosphine, $$\(\mathrm{PH}_{3}\)$$. This compound can react with a hydrogen ion, $$\(\mathrm{H}^{+}\)$$. Which type of interaction occurs between $$\(\mathrm{PH}_{3}\)$$ and $$\(\mathrm{H}^{+}\)$$?

Answer:

Knowledge points:

Solution:

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