Chemical Properties of Metals

Edited By Team Careers360 | Updated on Jul 02, 2025 04:48 PM IST

In this article we will discuss the properties of metals, chemical properties of metals, physical properties of metals, chemical properties of metals and non-metals. The arrangement of elements in a tabular form is known by the name periodic table and there are 115 elements present in the periodic table. There are many common features as well as different features in the properties of these elements. On this basis we can divide the elements into metals and non-metals. Metals are those elements which are present on the left hand side of the periodic table and generally are of five kinds of metals: Alkaline earth metals, Alkali metals, Transition metals, Actinides and Lanthanides.

NEET 2025: Mock Test Series | Syllabus | High Scoring Topics | PYQs

JEE Main: Study Materials | High Scoring Topics | Preparation Guide

JEE Main: Syllabus | Sample Papers | Mock Tests | PYQs

This Story also Contains

Metals:
Non-Metals:
Chemical Properties of Metals
Chemical Properties of Non-Metals:

Metals:

Metals are said to be those electropositive elements which are able to donate electrons and form positive charged ions known as protons and it will become stable in nature. The general reaction shown by any metal can be represented as:

1639366340155 , where M stands for any metal element.

The elements which show the properties represented by the metal are come in the category of metals. Physical properties of metals are described in this manner:

1. Metals are lustrous in nature.

2. They show malleability and ductility.

3. Sonorous in nature.

4. Good conductor of heat and electricity.

5. Generally solid at room temperature.

6. High melting and boiling point.

Also read -

Non-Metals:

Non-metals are said to be those elements which have tendency of accepting or gaining electrons to form negative ions. Non-metals shows 4-7 valence electrons i.e. electrons present in their outermost shell. It have high ionization energy and high electronegativity. Generally non-metals are said to be those substances which are not able to follow the properties of metals. The number of non-metals present in the periodic table are comparatively less than metals and non-metals are generally placed on the left side of the periodic table. These follows following properties:

1. Non-metals are said to be brittle and soft in nature.

2. These are poor conductor or we can termed non-metals as insulators.

3. Non-metals have no tendency to show those properties which are represented by metals like malleability, ductility etc.

And 22 non-metals are present in the periodic table.

Other than physical properties there are also some other properties called chemical properties of metals and non-metals/chemical properties of metals and nonmetals can be distinguished.

1. Reaction of metal with oxygen or reaction of metals with oxygen or Reaction of metal with air: Metals generally reacts with oxygen and form oxides known by the name metal oxides. These are of basic nature but metal oxides can also be amphoteric in nature. Amphoteric oxides are those which can behave as acid as well as basic oxides. The formation of metal oxide can be shown as:

Some metals are not fit to react with oxygen like two metals called sodium or potassium react very vigorously with oxygen and catches fire which is very dangerous and these metals are kept in kerosene oil.

2. Reaction of metal with water: When metals react with water then metal forms metal hydroxides but it is also seen that not all metals react with water. The tendency to react with water also varies from metal to metal. Metals known as sodium or potassium which reacts vigorously with oxygen are also very much reactive with water. When these metals reacts with water then it forms basic compounds or we can say alkalis. Reactions can be shown as:

a. Reaction of Sodium with water: Sodium combines with water and form sodium hydroxide and hydrogen gas which can be shown as:

b. Reaction of potassium with water: Potassium forms potassium hydroxide and hydrogen gas which can be represented as:

c. Reaction of calcium with water: Calcium when reacts with water form calcium hydroxide along with hydrogen gas which can be shown as:

Magnesium and zinc are the metals which are not able to react with cold water but can form oxides with hot water. It is the main point to remember that magnesium ad zinc form oxides with water not hydroxides. Reactions can be discussed as below

d. Reaction of magnesium with water: Magnesium forms oxides with water as compare to hydroxides and liberate hydrogen gas which can be shown as:

e. Reaction of zinc with water: Zinc also form oxide with water like magnesium and liberate hydrogen gas too. Reaction can be represented as:

Iron is very much less reactive as compare to sodium, potassium, calcium, magnesium and zinc so these are not able to react with cold as well as hot water. Iron reacts with steam and form magnetic oxides along with hydrogen gas which is represented as:

3. Reaction of metal with dilute acids: Highly reactive metals like sodium, potassium, lithium and calcium reacts very fast with dilute hydrochloric acid represented by and sulphuric acid represented by which forms salt of metal and also liberate hydrogen gas like reaction with water.

General reaction of metal with dilute hydrochloric acid can be shown as:

Reaction with dilute sulphuric acid can be shown as:

Where M represents metal ion.

Related Topics,

On the other hand the metals which are not much reactive like magnesium, zinc, iron, lead and tin not reacts vigorously with water but show slow reactions. Like magnesium when reacts with hydrochloric acid give reaction which is as follows:

While iron reacts with sulphuric acid and gives the reaction as follows:

Metals which are present below the hydrogen atom in the series known by the reactivity series generally not able to react with dilute acids. As they do not have tendency to displace hydrogen atom which further can form a bond with any non-metal anion.

4. Reaction of metal with other salts: Metals which are very reactive in nature can easily react with those metals which are less reactive in nature. In these type of reactions more reactive metal displace the less reactive one which further form oxides, chlorides or sulphides. Reaction of metal with salts can be represented as follows:

Which metals atom will replace which atom this will be explained on the basis of electrochemical series in which metals are arranged according to their electrode potential. Electrode potential is defined as the separation between the positive and negative charges at the stage called equilibrium state results in the difference between electrical potential of metal and the solution of its ions. The potential difference of the metal at the equilibrium state depends on the nature of metal, its ions, the concentration of ions and the temperature.

Electrochemical series can be shown as follows:

Elements reactivity series

Also, students can refer,

NEET Highest Scoring Chapters & Topics

This ebook serves as a valuable study guide for NEET exams, specifically designed to assist students in light of recent changes and the removal of certain topics from the NEET exam.

Download EBook

Chemical Properties of Non-Metals:

1. Reactions of non-metals with water: Non-metals not generally react with water but can react with air.

2. Non-metals reaction with acids: Non-metals also not react with any acids.

3. Reaction with bases: When non-metals reacts with basis it form very complex compounds like reaction of chlorine with base let us say sodium hydroxide gives product like sodium hypochlorite, sodium chloride along with water.

4. Non-metals with oxygen/ reaction of non metals with water: Non-metals generally form oxides when react with oxygen atoms. The oxides are mainly acidic or neutral in nature.

Like when sulphur reacts with oxygen it forms sulphur dioxide which can be shown as:

Also check-

NCERT Chemistry Notes:

Frequently Asked Questions (FAQs)

1. 1. Write three basis properties of metals?

1. Malleable

2. Ductile

3. Good conductor of heat and electricity.

2. 2. Define what is the product when non-metals react with water?

Non-metals do not react with water.

3. 3. Define ductility.

Ductility is that property of metals through which metals are molded into wires. Metals like aluminium, copper, silver are drawn into wires due to these properties.

4. 4. What happen when metal reacts with oxygen?

Metals generally react with oxygen and form oxides of metals along with the liberation of hydrogen gas.

5. 5. What is the product form when metals with water reacts?

Metals generally react with water and form hydroxides of metals.

6. Why do metals typically form positive ions?

Metals form positive ions because they have a tendency to lose electrons from their outermost shell. This is due to their low ionization energy and electronegativity, which makes it easier for them to give up electrons and achieve a stable electron configuration.

7. What is the significance of the activity series of metals?

The activity series of metals is a list that ranks metals in order of their reactivity. It is significant because it helps predict the outcomes of displacement reactions between metals and metal compounds. More reactive metals can displace less reactive metals from their compounds.

8. Why are some metals called "noble metals"?

Noble metals, such as gold, silver, and platinum, are called so because they are highly resistant to chemical reactions and corrosion. They have high ionization energies and electron affinities, making them less likely to form compounds or react with other elements.

9. Why do some metals react violently with water while others do not react at all?

The reactivity of metals with water depends on their position in the activity series. Highly reactive metals like sodium and potassium react violently with water because they easily lose electrons to form hydroxides and hydrogen gas. Less reactive metals like copper or gold do not react with water because their ionization energy is too high to allow electron transfer.

10. How does the atomic structure of metals contribute to their malleability and ductility?

The malleability and ductility of metals are due to their metallic bonding structure. In metals, the outer electrons are delocalized and form a "sea of electrons" around the positive metal ions. This allows the layers of metal atoms to slide over each other when force is applied, without breaking the overall structure.

11. What are the main differences between metals and non-metals in terms of their chemical properties?

Metals generally lose electrons to form positive ions, while non-metals gain electrons to form negative ions. Metals tend to be good conductors of heat and electricity, have a lustrous appearance, and are malleable and ductile. Non-metals are usually poor conductors, have a dull appearance, and are often brittle.

12. How do the reactivity trends differ between metals and non-metals in the periodic table?

For metals, reactivity generally increases from top to bottom in a group and from right to left across a period. For non-metals, reactivity typically increases from left to right across a period and from bottom to top in a group. This is due to differences in atomic size, ionization energy, and electron affinity.

13. How does the concept of electronegativity relate to the properties of metals and non-metals?

Electronegativity is the ability of an atom to attract electrons in a chemical bond. Non-metals generally have higher electronegativity values than metals. This difference explains why metals tend to lose electrons (forming cations) and non-metals tend to gain electrons (forming anions) in chemical reactions.

14. Why are some non-metals, like carbon and silicon, able to form long chains or networks?

Carbon and silicon can form long chains or networks due to their ability to covalently bond with themselves (catenation). This is possible because they have four valence electrons, allowing them to form stable, directional covalent bonds with other atoms of the same element or different elements.

15. What is meant by the term "metalloid," and how do metalloids differ from metals and non-metals?

Metalloids are elements that exhibit properties of both metals and non-metals. They are typically found along the diagonal line separating metals and non-metals on the periodic table. Metalloids can conduct electricity to some degree (unlike most non-metals) but are not as good conductors as metals. They also have intermediate electronegativity values.

16. How do alloys differ from pure metals in terms of their properties?

Alloys are mixtures of two or more elements, where at least one is a metal. They often have enhanced properties compared to pure metals, such as increased strength, hardness, or corrosion resistance. This is because the different-sized atoms in alloys can disrupt the regular crystal structure of pure metals, making it harder for layers to slide past each other.

17. What is the relationship between a metal's position in the periodic table and its melting point?

Generally, metals with higher melting points are found towards the middle of the periodic table (transition metals). This is due to their stronger metallic bonds resulting from multiple valence electrons. Alkali and alkaline earth metals, with fewer valence electrons, tend to have lower melting points.

18. What is the relationship between a metal's reactivity and its extraction method?

The reactivity of a metal determines the method used for its extraction. Highly reactive metals, like aluminum, require electrolysis for extraction because they form strong bonds with other elements. Less reactive metals, like copper, can be extracted by heating their ores with carbon (reduction). The least reactive metals, like gold, are often found in their pure form in nature.

19. What is the significance of the "inert pair effect" in the chemical properties of some heavy metals?

The inert pair effect refers to the tendency of the outermost s electrons in some heavy metals (like lead or tin) to resist participation in chemical bonding. This effect becomes more pronounced for heavier elements in a group and can lead to unexpected oxidation states or chemical behaviors in these metals.

20. How do transition metals differ from main group metals in terms of their chemical properties?

Transition metals can form multiple oxidation states due to their partially filled d-orbitals, leading to a wide range of colored compounds and complex ions. They also tend to form stronger metallic bonds, resulting in higher melting points and greater hardness compared to main group metals.

21. Why are some non-metals, like fluorine and oxygen, highly electronegative?

Fluorine and oxygen are highly electronegative due to their small atomic size and high effective nuclear charge. Their nuclei strongly attract electrons, and they need only a few electrons to achieve a stable octet configuration. This makes them very effective at attracting electrons in chemical bonds.

22. How does the concept of electron affinity relate to the chemical properties of non-metals?

Electron affinity is the energy change when an atom in the gas phase gains an electron. Non-metals generally have high electron affinities, meaning they release energy when gaining electrons. This property contributes to their tendency to form anions and their high electronegativity.

23. How does the concept of oxidation states relate to the behavior of metals and non-metals in chemical reactions?

Oxidation states represent the degree of oxidation of an atom in a compound. Metals typically have positive oxidation states because they tend to lose electrons in reactions. Non-metals often have negative oxidation states because they tend to gain electrons. This concept helps in understanding and balancing redox reactions involving metals and non-metals.

24. How do amphoteric oxides demonstrate the intermediate nature of some elements?

Amphoteric oxides can react as both acids and bases, depending on the reaction conditions. Elements that form amphoteric oxides (like aluminum or zinc) often lie near the dividing line between metals and non-metals on the periodic table, demonstrating properties intermediate between typical metals and non-metals.

25. Why do some metals form basic oxides while non-metals form acidic oxides?

Metal oxides tend to be basic because they can release OH- ions when dissolved in water. This is due to the metal's tendency to lose electrons, forming cations that attract OH- ions. Non-metal oxides are typically acidic because they can accept electron pairs from water molecules, releasing H+ ions.

26. How does the concept of electronegativity difference relate to the type of bonding between elements?

The electronegativity difference between two elements determines the type of bonding. A large difference (typically >1.7 on the Pauling scale) results in ionic bonding, where electrons are transferred. A small difference leads to covalent bonding, where electrons are shared. Intermediate differences result in polar covalent bonds.

27. What is the significance of the "diagonal relationship" in the periodic table?

The diagonal relationship refers to similarities in properties between certain elements diagonally adjacent in the periodic table (e.g., Li and Mg, Be and Al). This occurs because the opposing trends in atomic size and nuclear charge across a period and down a group can lead to similar properties for these pairs.

28. How do metals and non-metals differ in their ability to form hydrogen bonds?

Non-metals like nitrogen, oxygen, and fluorine can form hydrogen bonds due to their high electronegativity and small size, which creates a strong partial negative charge. Metals, having lower electronegativity, do not typically form hydrogen bonds, although they may participate in other types of intermolecular forces.

29. Why do some metals form colored compounds while others do not?

Colored metal compounds are typically formed by transition metals due to their partially filled d-orbitals. These d-orbitals can absorb light of specific wavelengths, resulting in the complementary color being observed. Main group metals, with fully filled or empty d-orbitals, usually form colorless compounds.

30. How does the concept of lattice energy relate to the properties of ionic compounds formed by metals and non-metals?

Lattice energy is the energy required to separate one mole of an ionic solid into gaseous ions. Higher lattice energies result in stronger ionic bonds and more stable compounds. Lattice energy increases with increasing charge on the ions and decreasing ion size, affecting properties like melting point and solubility.

31. What is the "lanthanide contraction," and how does it affect the properties of transition metals?

The lanthanide contraction is the decrease in atomic and ionic radii across the lanthanide series due to poor shielding by 4f electrons. This contraction affects the size of elements in subsequent periods, leading to unexpected similarities in properties between certain pairs of transition metals (e.g., Zr and Hf).

32. How do metals and non-metals differ in their ability to form coordination compounds?

Metals, especially transition metals, readily form coordination compounds by accepting electron pairs from ligands into their empty orbitals. Non-metals typically do not form coordination compounds because they lack suitable empty orbitals to accept electron pairs.

33. Why do some metals form multiple oxidation states while others do not?

Metals that form multiple oxidation states, typically transition metals, have partially filled d-orbitals. These d-electrons can be easily lost or shared in bonding, allowing for various oxidation states. Main group metals with stable electron configurations (like Na+ or Mg2+) tend to form only one common oxidation state.

34. How does the concept of Pearson's HSAB (Hard and Soft Acids and Bases) theory apply to metal-ligand interactions?

Pearson's HSAB theory classifies metal ions (acids) and ligands (bases) as hard or soft. Hard acids (small, highly charged metal ions) prefer to bind with hard bases (small, highly electronegative ligands), while soft acids (large, low-charged metal ions) prefer soft bases (large, polarizable ligands). This theory helps predict the stability of metal complexes.

35. What is the significance of the "spectrochemical series" in understanding metal complex properties?

The spectrochemical series ranks ligands based on their ability to cause d-orbital splitting in metal complexes. This splitting affects the color, magnetic properties, and stability of complexes. Understanding the series helps predict and explain the properties of different metal-ligand combinations.

36. How do the principles of hard-soft acid-base (HSAB) theory relate to the reactivity of metals and non-metals?

HSAB theory classifies metals (acids) and non-metals (bases) as hard or soft based on their polarizability. Hard acids (small, highly charged metals) prefer to react with hard bases (small, highly electronegative non-metals), while soft acids (large, low-charged metals) prefer soft bases (large, polarizable non-metals). This theory helps predict the stability and reactivity of various compounds.

37. Why do some metals form amalgams while others do not?

Amalgams are alloys of mercury with other metals. Metals that readily form amalgams (like silver, gold, and zinc) can dissolve in mercury due to favorable interactions between their atoms and mercury atoms. Metals that don't form amalgams (like iron) have stronger interatomic bonds that resist dissolution in mercury.

38. How does the concept of electronegativity explain the trend in acid-base properties of oxides across a period?

As we move from left to right across a period, the electronegativity of elements increases. This leads to a gradual change in the nature of oxides from basic (metal oxides) to amphoteric (e.g., Al2O3) to acidic (non-metal oxides). Higher electronegativity results in stronger covalent bonds between the element and oxygen, increasing the acidity of the oxide.

39. What is the "trans effect" in coordination compounds, and how does it influence ligand substitution reactions?

The trans effect is the ability of certain ligands to labilize (weaken) the bond of the ligand trans to them in square planar or octahedral complexes. Ligands with strong trans effects (like CO or CN-) facilitate substitution reactions of the trans ligand. This concept is crucial in understanding the kinetics and mechanisms of ligand substitution reactions in metal complexes.

40. How do the concepts of electronegativity and atomic size explain the diagonal relationship in the periodic table?

The diagonal relationship refers to similarities in properties between elements diagonally adjacent in the periodic table (e.g., Li and Mg, Be and Al). This occurs because the decrease in atomic size across a period is roughly compensated by the increase in atomic size down a group, resulting in similar charge density and electronegativity for diagonally related elements.

41. Why do some metals form interstitial compounds, and how do these compounds affect the properties of the metal?

Interstitial compounds form when small non-metal atoms (like H, C, or N) occupy the interstitial spaces in a metal's crystal lattice. This occurs in metals with larger atomic radii, typically transition metals. Interstitial compounds often increase the hardness and melting point of the metal while decreasing its ductility and electrical conductivity.

42. How does the concept of electron configuration explain the magnetic properties of transition metal complexes?

The magnetic properties of transition metal complexes depend on the number of unpaired electrons in the d-orbitals. High-spin complexes (with more unpaired electrons) are paramagnetic, while low-spin complexes (with fewer unpaired electrons) can be diamagnetic. The electron configuration, influenced by the strength of the ligand field, determines whether a complex is high-spin or low-spin.

43. What is the significance of Fajan's rules in predicting the covalent character of predominantly ionic compounds?

Fajan's rules predict the degree of covalent character in predominantly ionic compounds. They state that covalent character increases with: 1) increasing charge on the cation, 2) decreasing size of the cation, and 3) increasing polarizability of the anion. These rules help explain why some compounds expected to be ionic show some covalent properties.

44. How does the lanthanide contraction affect the properties of post-transition metals?

The lanthanide contraction, caused by poor shielding of 4f electrons, results in a smaller than expected increase in atomic radius from the 5d to 6d elements. This leads to similar atomic sizes and properties between 4d and 5d elements (e.g., Zr and Hf). It also affects the properties of post-transition metals, influencing their reactivity, ionization energies, and atomic radii.

45. Why do some non-metals, like sulfur, exhibit allotropy, and how does this affect their properties?

Allotropy is the existence of an element in multiple structural forms. Some non-metals, like sulfur, exhibit allotropy due to their ability to form different molecular structures or crystal lattices. Different allotropes can have vastly different properties (e.g., rhombic vs. monoclinic sulfur) due to variations in bonding and molecular arrangement.

46. How does the concept of electron affinity explain the trend in halogen reactivity?

Electron affinity generally increases across a period due to increasing nuclear charge and decreasing atomic size. Halogens have the highest electron affinities in their respective periods, with fluorine having the highest overall. This trend explains why fluorine is the most reactive halogen, as it most readily accepts an electron to form a stable anion.

47. What is the "chelate effect," and how does it influence the stability of metal complexes?

The chelate effect refers to the increased stability of metal complexes containing multidentate ligands (chelating agents) compared to similar complexes with monodentate ligands. This increased stability is due to entropy factors and the formation of multiple coordinate bonds between the metal and a single ligand molecule, making the dissociation of the complex less likely.

48. How do the concepts of atomic radius and ionization energy explain the trend in metallic character across the periodic table?

Metallic character generally decreases across a period and increases down a group. This trend is explained by decreasing atomic radius and increasing ionization energy across a period, making it harder for atoms to lose electrons. Down a group,