Thus, we will think of these bonds in the following order (strongest to weakest): Covalent, Ionic, Hydrogen, and van der Waals.

Chemical bonds also influence such other properties as crystal symmetry and cleavage. Stronger bonds between atoms make them more difficult to separate and, in general, stronger chemical bonds result in greater hardness, higher melting and boiling points, and smaller coefficients of expansion.

Two or more of these bond types can and do coexist in most minerals. Covalent bonds are very strong bonds formed when atoms share electrons with neighboring atoms. Sulfur, and both of carbon’s natural forms, graphite and diamond, are covalently-bonded minerals….Chemical Bonding.

So, in summary, mineral strength is diagnostic in identifying a material and can be measured in different ways. Tenacity is the resistance of a mineral to breaking, and tenacity can be characterized as brittle, malleable, sectile and elastic.

1: The Strength of Covalent Bonds Depends on the Overlap between the Valence Orbitals of the Bonded Atoms. The relative sizes of the region of space in which electrons are shared between (a) a hydrogen atom and lighter (smaller) vs.

ionic bond

Covalent bond

The longest covalent bond I can find is the bismuth-iodine single bond. The order of bond lengths is single > double > triple. The largest atoms should form the longest covalent bonds. So we look at atoms in the lower right corner of the Periodic Table.

Ionic bond is generally stronger because the ion-ion force that exists in ionic bonding is the strongest. In covalent bonds, electrons are shared, which doesn’t generate a force as strong as that in ionic bonding. This can also be explained when we compare the boiling points of ionic compounds and covalent compounds.

As fluorine has small size and high electronegativity, it has high tendency to attract partial positive charge accumulated on H-atom. So, fluorine forms strongest H-bond.

Weakest hydrogen bond will be formed when the electronegativity difference between the atom and H is the least. Hence, S−H−−−−−H form the weakest hydrogen bond.

The hydrogen bond in HF is strongest , because fluorine is the most electronegative element .

Key Points

1. Hydrogen bonds are strong intermolecular forces created when a hydrogen atom bonded to an electronegative atom approaches a nearby electronegative atom.
2. Greater electronegativity of the hydrogen bond acceptor will lead to an increase in hydrogen-bond strength.

In order from strongest to weakest, the intermolecular forces given in the answer choices are: ion-dipole, hydrogen bonding, dipole-dipole, and Van der Waals forces.

The strongest hydrogen bond type is the one involving a bond between oxygen, nitrogen and fluorine, with a hydrogen atom. Since in the choices, only water shows a O-H bond, therefore this is the strongest hydrogen bonding. The answer is water.

Dipole-dipole interactions

London dispersion force

Actually, gravity is the weakest of the four fundamental forces. Ordered from strongest to weakest, the forces are 1) the strong nuclear force, 2) the electromagnetic force, 3) the weak nuclear force, and 4) gravity.

Liquid helium

water

A liquid at high pressure has a higher boiling point than when that liquid is at atmospheric pressure. For example, water boils at 100 °C (212 °F) at sea level, but at 93.4 °C (200.1 °F) at 1,905 metres (6,250 ft) altitude. For a given pressure, different liquids will boil at different temperatures.

2-methylpropane

• Answer : 0.1 M of NaCl has the higher boiling point.
• Explanation :
• Formula used for Elevation in boiling point :
• As per question, we conclude that the molality of the given solution are same.
• Now we have to calculate the Van’t Hoff factor for the given solutions.
• Hence, 0.1 M of NaCl has the higher boiling point.

Which will have higher boiling point, 0.1 M NaCl or 0.1 M BaCl2 solution In water and why ? Since both the salt solution have same concentration, therefore the salt which gives maximum number of ions will show higher boiling point. NaCl dissociate to give two ions while BaCl. Hence BaCl2 posses high boiling point.

0.1 M CaCl_(2) has higher boiling point than 0.1 M NaCl. Vapour pressure of 0.05 M urea solution is greater than that of 0.05 M KCl solution.

• 0.1 M MgCl2. B.
• 0.1 M HClO4. C.
• 0.1 M KCl. D.
• 0.1 M KOH. E.
• 0.1 M LiNO3. Medium. Answer. Correct option is.
• 0.1 M MgCl2. 0.1 M MgCl2 solution has the highest boiling point. Elevation in the boiling point is a colligative property and depends on the number of solute particles.

• 1 M NaCl. B.
• 1 M urea. C.
• 1 M BaCl2. D.
• 1 M glucose. Medium. Answer. Correct option is. C.
• 1 M BaCl2. The right answer is 0. 1M BaCl2 has the highest boiling point. Barium chloride solution contains the greatest number of solute particles.