notes on metals and non-metals. include their properties, reactivity and their arrangements on the periodic table
Metals:
1. Properties:
- Shiny luster
- Good conductors of heat and electricity
- Malleable and ductile (can be hammered into thin sheets and drawn into wires)
- High density and melting points
- Generally solid at room temperature (except for mercury, which is a liquid)
- Form positive ions by losing electrons in chemical reactions
2. Reactivity:
- High reactivity: alkali metals (Group 1) and alkaline earth metals (Group 2) are highly reactive and easily lose electrons to form positive ions.
- Moderate reactivity: transition metals (Groups 3-12) have varying reactivity, but generally form positive ions.
- Low reactivity: noble metals (such as gold and platinum) are highly unreactive and do not readily lose electrons.
3. Arrangement on the periodic table:
- Majority of metals are found on the left-hand side of the periodic table.
- They are located in Groups 1 to 12, as well as in the d-block (transition metals) and f-block (lanthanides and actinides).
Non-Metals:
1. Properties:
- Dull or non-shiny appearance (exception: iodine and graphite)
- Poor conductors of heat and electricity
- Brittle and non-malleable (cannot be hammered into thin sheets or drawn into wires)
- Low density and melting points
- Various physical states at room temperature (solid, liquid, or gas)
- Form negative ions by gaining electrons or share electrons in chemical reactions (except for hydrogen, which can form positive ions)
2. Reactivity:
- High reactivity: halogens (Group 17) are highly reactive non-metals and readily gain electrons to form negative ions.
- Moderate reactivity: non-metals in Group 16 (oxygen, sulfur, etc.) have moderate reactivity and readily form negative ions.
- Low reactivity: noble gases (Group 18) are considered non-reactive as they have completely filled electron shells and do not readily gain or lose electrons.
3. Arrangement on the periodic table:
- Non-metals are mostly found on the right-hand side of the periodic table.
- They are located in Groups 14 (carbon, silicon, etc.) to 18 (helium, neon, etc.), as well as in the p-block.
Metals and non-metals are two broad categories of elements on the periodic table. Let's discuss their properties, reactivity, and their arrangements on the periodic table step-by-step:
Properties of Metals:
1. Physical Properties:
- Metals are generally shiny and have a metallic luster.
- They are malleable, meaning they can be hammered or rolled into thin sheets.
- Metals are ductile, meaning they can be drawn into thin wires.
- They have high melting and boiling points.
- Metals are good conductors of heat and electricity.
2. Chemical Properties:
- Most metals tend to lose electrons and form positive ions (cations) when they undergo chemical reactions.
- Metals typically have a tendency to form ionic compounds.
- They react with oxygen to form metal oxides.
- Metals generally react with acids to produce hydrogen gas.
Reactivity of Metals:
1. Reactivity Series:
- Metals can be arranged in a reactivity series, where the most reactive metals are at the top and the least reactive at the bottom.
- The reactivity of metals generally increases as you move up the series.
- Alkali metals such as potassium and sodium are extremely reactive, while noble metals like gold and platinum are relatively unreactive.
2. Factors Influencing Reactivity:
- The reactivity of metals is influenced by factors such as the tendency to lose electrons, atomic size, and ionization energy.
- Generally, metals with low ionization energy and large atomic size are more reactive.
Arrangement of Metals on the Periodic Table:
1. Location:
- Metals are found primarily on the left side of the periodic table.
- Transition metals are located in the middle of the periodic table.
2. Groups:
- Metals are found in various groups on the periodic table.
- Group 1 elements are known as alkali metals (e.g., lithium, sodium).
- Group 2 elements are called alkaline earth metals (e.g., magnesium, calcium).
Properties of Non-Metals:
1. Physical Properties:
- Non-metals are generally dull and have a non-metallic luster.
- They are brittle and cannot be shaped into thin sheets or drawn into wires.
- Non-metals have low melting and boiling points.
- They are poor conductors of heat and electricity.
2. Chemical Properties:
- Non-metals tend to gain electrons and form negative ions (anions) when they undergo chemical reactions.
- Non-metals generally form covalent compounds.
- They react with oxygen to form non-metal oxides.
- Non-metals may react with acids but do not produce hydrogen gas.
Reactivity of Non-Metals:
1. Reactivity:
- Non-metals vary in their reactivity.
- Some non-metals, like fluorine and chlorine, are highly reactive, while others such as carbon and sulfur are less reactive.
2. Factors Influencing Reactivity:
- Non-metal reactivity is influenced by factors such as electronegativity and electron affinity.
- Generally, non-metals with high electronegativity and electron affinity are more reactive.
Arrangement of Non-Metals on the Periodic Table:
1. Location:
- Non-metals are primarily located on the right side of the periodic table.
- They are found in groups 14, 15, 16, and 17.
2. Groups:
- Group 17 elements are known as halogens (e.g., fluorine, chlorine).
- Group 18 elements are noble gases (e.g., helium, neon).
In summary, metals have properties such as shiny appearance, malleability, and are good conductors of heat and electricity. They tend to lose electrons, become cations, and react in various ways with other elements. Non-metals, on the other hand, are generally dull in appearance, have low melting points, and poor conductivity. They tend to gain electrons, become anions, and have their own unique chemical reactions. Their arrangement on the periodic table can be observed based on the location, groups, and reactivity patterns.