Melting point is the temperature at which any solid changes its form from solid to liquid. The melting point of any solid is the temperature at which it changes its temperature from solid to liquid at constant pressure, (generally at constant pressure). At the melting point, the liquid and solid phases of any material exist simultaneously.
In this article, we will learn about melting points and various factors that affect melting points, examples, and others in detail.
What is Melting Point?
The temperature at which a solid substance melts and transforms into a liquid at atmospheric pressure is termed the melting point of a substance.
Different solids display varying melting points. For example, the melting point of wax is 63 °C. The greater the melting point of the substances, the more will be the intraparticle forces of attraction binding the particles. For instance, in the solid form of water, ice melts at a temperature of 0 °C to form liquid water. Therefore, the melting point of ice is 0 °C at atmospheric pressure.
At the melting point, the solid and liquid states of matter coexist together. The melting point of a substance is its characteristic property influenced by the applied pressure.
Explanation of Melting Point
Melting or fusion is the process by which a solid substance changes into a liquid on heating. On heating a substance, the particles vibrate with greater intensity and move more vigorously. Heat energy is produced. The particles gain sufficient kinetic energy to overcome the strong forces of attraction. They gain energy to break through to form small groups of particles. Solids, therefore, melt to form a liquid state.
Melting of a substance occurs at defined ambient pressure conditions. The energy supplied to melt a system is known as Enthalpy of fusion or Entropy of fusion. However, some of the substances pose an exception to this process, and heat has to be removed from these systems in order to melt them. e.g. Helium.
Melting Point Determination Methods
In chemistry labs, there are various methods for the determination of melting points.
- Simple Melting Point Apparatus
- Automated Melting Point Apparatus
- Capillary Tube Method
Factors Affecting Melting Point
Molecular Structure and Intermolecular Forces
As the Melting point is the point at which atoms release themselves from the intermolecular forces using the energy of the surroundings, thus molecular structure and intermolecular forces affect the melting point. Substances with stronger intermolecular forces, such as hydrogen bonding or dipole-dipole interactions, tend to have higher melting points. For example, water (H2O) has strong hydrogen bonding, leading to a relatively high melting point.
Molecular Weight and Size
Larger the molecule, the more area it has for intermolecular interactions, hence a much stronger force of attraction between molecules and melting point as well. Therefore, larger molecules have greater melting points than smaller molecules. Other than size, shape also affects the melting point as linear-shaped molecules can be packed much more efficiently than branched or spherical-shaped molecules.
Impurities and Purity of Substances
The presence of impurities in a substance can lower its melting point. Impurities disrupt the regular packing arrangement of molecules or ions, making it easier for the substance to transition from the solid to the liquid phase. This phenomenon is known as "melting point depression."
Common Examples of Melting Points
There are various common daily-use compounds, for which we will discuss the melting point.
Metals
The melting point of some most common metals are:
Chemical | Melting Point (K) | Melting Point (°C) |
|---|
| Sodium (Na) | 370.87 | 97.87 |
|---|
| Magnesium (Mg) | 923 | 650 |
|---|
| Aluminium (Al) | 933.47 | 660.47 |
|---|
| Potassium (K) | 336.53 | 63.53 |
|---|
| Titanium (Ti) | 1941 | 1668 |
|---|
| Iron (Fe) | 1811 | 1538 |
|---|
| Nickel (Ni) | 1728 | 1455 |
|---|
| Copper (Cu) | 1357.77 | 1084.77 |
|---|
| Zinc (Zn) | 692.88 | 419.88 |
|---|
| Gallium (Ga) | 302.9146 | 29.9146 |
|---|
| Silver (Ag) | 1234.93 | 961.93 |
|---|
| Cadmium (Cd) | 594.22 | 321.22 |
|---|
| Indium (In) | 429.75 | 156.75 |
|---|
| Tungsten (W) | 3695 | 3422 |
|---|
| Platinum (Pt) | 2041.4 | 1768.4 |
|---|
| Gold (Au) | 1337.33 | 1064.33 |
|---|
| Mercury (Hg) | 234.43 | -38.57 |
|---|
| Lead (Pb) | 600.61 | 327.61 |
|---|
| Bismuth (Bi) | 544.7 | 271.7 |
|---|
Non-Metals
The melting point of some most common non-metals are:
Element | Melting Point (K) | Melting Point (°C) |
|---|
| Hydrogen (H) | 14 | -259 |
|---|
| Nitrogen (N) | 63.15 | -209.85 |
|---|
| Oxygen (O) | 54.36 | -218.64 |
|---|
| Sulfur (S) | 388.36 | 115.36 |
|---|
| Chlorine (Cl) | 171.6 | -101.4 |
|---|
| Iodine (I) | 386.85 | 113.85 |
|---|
Organic Compounds
The melting point of some most common organic compounds are:
Chemical | Melting Point (K) | Melting Point(°C) |
|---|
| Methane(CH4) | 109 | -164 |
|---|
| Ethane(C2H6) | 184 | -89 |
|---|
| Methanol (CH3OH) | 338 | 65 |
|---|
| Propane (C3H8) | 231 | -42 |
|---|
| Ethanol (C2H5OH) | 351 | 78 |
|---|
| Butane (C4H10) | 272 | -1 |
|---|
| Phenol (C6H6O) | 315 | 42 |
|---|
| Oxalic Acid (C2H2O4) | 374 | 101 |
|---|
| Benzoic Acid (C7H6O2) | 395 | 122 |
|---|
| Naphthalene (C10H10) | 353 | 80 |
|---|
| Fructose (C6H12O6) | 376 | 103 |
|---|
| Glucose (C6H12O6) | 419 | 146 |
|---|
| Sucrose (C12H22O11) | 459 | 186 |
|---|
Inorganic Compounds
The melting point of some most common inorganic compounds are:
Compound | Melting Point (°C) | Melting Point (K) |
|---|
| Water (H2O) | 0 | 273 |
|---|
| Sodium Chloride (NaCl) | 801 | 1074 |
|---|
| Calcium Carbonate (CaCO3) | 825 | 1098 |
|---|
| Aluminum Oxide (Al2O3) | 2072 | 2345 |
|---|
| Silicon Dioxide (SiO2) | 1713 | 1986 |
|---|
| Copper (Cu) | 1083 | 1356 |
|---|
| Iron (Fe) | 1538 | 1811 |
|---|
| Lead (Pb) | 327.5 | 600.5 |
|---|
| Zinc (Zn) | 419.5 | 692.5 |
|---|
| Silver (Ag) | 961.8 | 1234.8 |
|---|
| Gold (Au) | 1064 | 1337 |
|---|
| Mercury (Hg) | -38.83 | 234.17 |
|---|
| Carbon Dioxide (CO2) | -78.5 | 194.5 |
|---|
| Ammonium Nitrate (NH4NO3) | 169.6 | 442.6 |
|---|
Check: Melting Point and Boiling Point
Applications of Melting Point
The application can be observed during the process of snow skating. The weight of the skater gets concentrated on a thin line, there is considerable pressure applied on the ice slab. This results in the melting of ice beneath the shoe of the skater. This melting ice lubricates the undersides of his skating shoes. This makes it possible to skate on the ice.
Conversion of Solid to Liquid
The process of a solid turning into a liquid state is called melting. It is also known as fusion. The reverse process of a liquid becoming a solid is in turn called solidification.
The temperature at which melting occurs for any pure substance is termed the melting point of that substance. Melting point is considered to be a physical characteristic of any substance. To melt a substance from solid to liquid, there is always a requirement of energy and as it requires energy, it is an endothermic reaction. Every pure substance requires a certain amount of energy which is required to change from a solid to a liquid state.
Energy is exclusively required to carry out the transition of the substance, from solid to liquid substance. The phase of a substance is changed, and the temperature remains unchanged. Therefore, melting is known to be an isothermal process, since the substance remains at the same unmodified temperature.
Check: Thermal Properties of Matter
Heating Curve for the Conversion of Solid to Liquid
The heating curve denotes the temperature on the y-axis and the heat that has been supplied on the x-axis respectively. Let us assume a constant rate of heating, owing to which the x-axis can be shown as the amount of time that is shown as the substance is being heated. The curve majorly shows two main points:
- The portion of the graphs, where the temperature rises as and when heat is supplied to the system, and
- The portion of the graphs plateaus where the temperature remains at a constant level. Change in phase occurs at this plateau.
Read More,
Sample Questions on Melting Point
Question 1: What causes phase change?
Answer:
When the temperature or pressure change of a system occurs, the phase changes. Upon increasing the temperature or pressure of the system, the intramolecular forces of attraction increase. Upon decreasing the temperature, the molecules or atoms turn into a rigid structure.
Question 2: Does temperature change during the process of heating ice?
Answer:
As we constantly supply heat energy to transform ice into water, the temperature of the system doesn't change. The heat energy is absorbed by the ice changing slowing into the liquid state. Both the states of matter coexist together during this process.
Question 3: How does melting occur in the case of amorphous solids?
Answer:
The non-crystalline solids, such as glass or pitch undergo melting by slowly decreasing viscosity with the simultaneous increase in the temperature. However, there is no sharp transformation from solid to liquid state.
Question 4: Define the heat of fusion.
Answer:
The amount of energy required by a pure substance to change from the solid to a liquid state is termed as the enthalpy of fusion (or heat of fusion) of the substance. It is denoted by ΔHfus.
Question 5: Differentiate between boiling and melting.
Answer:
Boiling is the process of melting of liquid to gas state whereas melting is the transformation of solid to liquid state.
Question 6: How does energy change occur during melting?
Answer:
Heat must be supplied to the enclosed system in order to simulate the melting of the substance. When energy is supplied the atoms composing the substance break away and are pulled apart farther.
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Drawbacks of Dalton's Atomic TheoryThe idea of atoms dates back two millennia, long before John Dalton introduced the concept of atoms in 1803. Kanada, an ancient Indian philosopher, discussed the existence of indivisible particles, which he referred to as "anu." The rule of conservation of matter was introduced by French scientist L
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Significance of the Symbol of ElementsAn element in chemistry refers to the purest form of a substance containing only atoms and cannot be broken down further by any means. These elements are classified according to their properties (both chemical and physical) and arranged according to their atomic number (Z) in the modern periodic tab
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Difference Between Molecules and CompoundsMolecules are the smallest building blocks that form the matter around us. They are the simplest particles that carry the properties of matter. Molecules are joined together to form the Compound. A molecule is the smallest unit of matter formed by joining various atoms together whereas the compounds
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How to Calculate Valency of Radicals?To construct the formulas of ionic compounds, we must first understand the valencies of the positive and negative ions that combine to produce the ionic compounds. As a result, we'll start with ion valencies. The valency of an ion is equal to its charge. If an ion has one unit charge, its valency is
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What is the Significance of the Formula of a Substance?Everyone may think that if the atom is very tiny in size, what is its importance of it? So, this is because the entire world is made up of atoms and molecules. As known that one cannot see them with the naked eyes but they are always present around. They may be in the surrounding, substances that ev
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Gram Atomic and Gram Molecular MassAvogadro's number is critical to understanding the structure of molecules as well as their interactions and combinations. e.g. because one atom of oxygen will combine with two atoms of hydrogen to form one molecule of water (H2O), one mole of oxygen (6.022 × 1023 of O atoms) will mix with two moles
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Chapter 4: Structure of the Atom
Charged Particles in MatterCan we deduce from these actions that rubbing two items together causes them to become electrically charged? The presence of charged particles in an atom was discovered thanks to the efforts of many scientists. By 1900, it was established that the atom was an indivisible particle that contained at l
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What is Atom?Atoms are tiny particles that comprise all the things in the known universe. Atoms of an element are responsible for all chemical reactions occurring in nature. We know that atoms are made up of three fundamental particles namely, ElectronsProtonsNeutronsThese particles are also called subatomic par
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Thomson's Atomic ModelThomson's Atomic Model is one of the fundamental models of the atom that tries to explain the working and structure of the atom. this model was proposed by famous Scientist JJ Thomson in 1904. Thomson during his cathode ray experiment proved the existence of a negatively charged particle called elec
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Rutherford Atomic ModelRutherford Atomic Model was proposed by Ernest Rutherford in 1911. It is also called the Planetary Model of the Atom. It introduced the concept of a dense, positively charged nucleus at the center of an atom, with electrons orbiting around it, forming the basis for modern atomic theory. In this arti
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Drawbacks of Rutherford's Atomic ModelIn Rutherford's Model of the Atom, Rutherford performed an experiment based on that experiment some of the hypotheses are given. At that time those hypotheses are considered revolutionary as there was an experiment to back that hypothesis. But as the experiment performed by Rutherford is rudimentary
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Bohr's Model of an AtomNeil Bohr proposed the Bohr model and was based on the modification of Rutherford’s model of an atom. Rutherford's model introduced a nuclear model of an atom in which it was explained that the nucleus which is positively charged is surrounded by negatively charged particles called electrons. Bohr m
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NeutronsNeutrons are fundamental subatomic particles of the atom. An atom is made up of electrons, protons and neutrons. James Chadwick, an English physicist, discovered the neutron in 1932. Neutrons are particles with no charge and higher mass. They are represented by n. They reside inside the nucleus of t
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ValencyValency of an element is a measure of an atom's ability to combine with other atoms to create molecules or chemical compounds. The characteristics of an element that indicate how many more atoms can join one of its atoms in a covalent bond are known as valence, or valency, in chemistry. The term, wh
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Valence ElectronsAny of the fundamental negatively charged particles in the outermost area of atoms that participate in the creation of chemical bonds are referred to as valence electrons. Changes in the atomic structure are confined to the outermost, or valence, electrons regardless of the kind of chemical connecti
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Mass NumberMass Number of an atom is the total number of protons and neutrons present in an atom. We know that an atom consists of electrons, protons, and neutrons but the mass of the atom is contributed by protons and neutrons as the mass of electrons is very low hence it doesn't contribute to the mass of an
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Relation Between Mass Number and Atomic NumberAtoms are the fundamental building blocks of matter, and they may combine in a variety of ways to produce various substances. You must be aware that all atoms are made up of electrons, protons, and neutrons. But did you know that the presence of these subatomic particles may explain an element's pro
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IsobarsIsobars are a group of elements that have the same mass number but different atomic numbers. In an isobar, we have different numbers of protons but the same number of nucleons, i.e. the sum of the number of protons and neutrons in the nucleus of isobars of the elements are the same. An example of is
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Why do all the Isotopes of an Element have similar Chemical Properties?The fundamental building units of matter are atoms and molecules. The existence of many types of matter is due to the various atoms that contain them. The atom was no longer seen as a simple, indivisible unit by 1900. It did, however, contain at least one subatomic particle, the electron. J.J. Thoms
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Why Isotopes have different Physical Properties?The atom is divided into two parts: the atomic structure and the extra nucleus. Positively charged protons and neutral neutrons make up the atomic structure. Electrons in the extra nucleus are negatively charged. Atoms, like all elements and compounds, have mass. Because of protons, the mass of an a
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What is Fractional Atomic Mass?The smallest possible amount of matter which still retains its identity as a chemical element, consisting of a nucleus surrounded by electrons is called an atom. These are the atoms that make up an element. An element is a material with the same number of protons in all of its atoms. Protons, electr
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Radioactive IsotopesRadioactive Isotopes or Radioisotopes are the isotopes of the elements that are not stable, i.e. they emit some radiation and change the composition of their nucleus. Radioactive isotopes are defined as the isotopes of any chemical element that have different masses and unstable nuclei and release e
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Discovery of ElectronsThe basic idea of the discovery of the elementary particles was generated by Dalton's Atomic Theory. John Dalton in 1808 gave the first scientific theory about atoms, in which, he stated that atoms are the smallest particle of any matter. They are indivisible and indestructible. According to Dalton
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What is a Proton?Protons are the fundamental particles that reside inside the nucleus of any atom. They are the positive charge particle and are responsible for balancing the negative charge of the electron to make the atom electrically neutral. Proton was discovered by the famous scientist Ernest Rutherford. Atoms
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Rutherford's Alpha Scattering ExperimentRutherford's Alpha Scattering Experiment is the fundamental experiment done by Earnest Rutherford's Alpha Scattering Experiment that gives the fundamental about the structure of the atom. Rutherford in his experiment directed high-energy streams of α-particles from a radioactive source at a thin she
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Atomic NucleusThe nucleus of an atom is a small, dense, round region located in the centre of an atom. It has two subatomic particles, protons and neutrons. Protons are electrically positively charged ions having a mass of approximately one atomic mass unit (amu). Neutrons are electrically neutral.The atomic nucl
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How did Neil Bohr explained the Stability of Atom?Bohr model of the atom was explained by Neil Bohr in 1915. It came into existence with the modification of Rutherford’s model of the atom. Rutherford’s model introduces the nuclear model of the atom, in which he explained that a nucleus (positively charged) is surrounded by negatively charged electr
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Electron ConfigurationElectron Configuration of an element tells us how electrons are filled inside various orbitals of the atom. The distribution of electrons inside various orbital of atoms is very useful in explaining various properties of the atoms and their combination with other atoms. The electron configuration of
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Potassium and Calcium - Atomic Structure, Chemical Properties, UsesAn atom is the smallest part of an element or compound that takes part in a chemical reaction. They are made of tiny particles known as protons, neutrons, and electrons. The Greek philosopher Democritus was the first person to use the term atom. The structure of the atom was discovered by John Dalto
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Noble GasInert gases are chemically unreactive. Noble gases, also termed inert gases are group 0 elements. There are six types of noble gases, helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and radioactive radon (Rn). The noble gases are the type of elements belonging to group 18. Under standa
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What is meant by Chemical Combination?The composition of an element's nucleus and the arrangement of electrons around it are referred to as its atomic structure. Protons, electrons, and neutrons are the building blocks of matter's atomic structure. The nucleus of the atom is made up of protons and neutrons, which is surrounded by the at
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Difference between Electrovalency and CovalencyWe're all familiar with how electrons in an atom are organised into orbitals or shells. Valence electrons are the electrons that exist in the atom's outermost orbit. According to the Bohr-bury theory, the outermost shell may hold a maximum of 8 electrons. When the outermost shell is entirely filled,
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