Difficulty: Beginner | Prerequisites: Basic understanding of the periodic table layout (groups and periods).
This is the first of three sections covering Chapter 17: Elements and Their Properties. Part 1 focuses on metals, which make up the majority of elements on the periodic table. You will need to know what metals are, how metallic bonding works, and the key families of metals (alkali, alkaline earth, transition). If you can already locate the stair-step line on the periodic table, you are in good shape. If not, review a labelled periodic table before reading on.
Metals are shiny, malleable, ductile elements that conduct heat and electricity well. They sit to the left of the stair-step line on the periodic table. The three main families, alkali metals (Group 1), alkaline earth metals (Group 2), and transition metals (Groups 3 to 12), differ in reactivity and electron configuration, but all tend to lose electrons and form positive ions.
Metal
An element that is shiny, malleable, ductile, and a good conductor of heat and electricity. In simple terms, metals are the elements that look and behave the way you picture a "typical" element: solid, shiny, bendable.
Malleable
Capable of being hammered or rolled into thin sheets without breaking. Think of it as: you can flatten it with a hammer and it will not shatter.
Ductile
Capable of being drawn out into a thin wire. In simple terms, if you can pull it into a long, thin strand (like copper wire), it is ductile.
Metallic bonding
A type of bonding in which positively charged metal ions are surrounded by a "sea" of freely moving electrons. Think of it as: the metal atoms share their outermost electrons in a communal pool, which is why metals conduct electricity and can bend without breaking.
Ionic bond
A bond formed when a metal transfers one or more electrons to a nonmetal, creating oppositely charged ions that attract each other. In simple terms, the metal gives electrons away, the nonmetal takes them, and the two stick together because of opposite charges.
Alkali metal
Any element in Group 1 of the periodic table (excluding hydrogen). These are the most reactive metals and have one electron in their outermost energy level. Think of it as: the leftmost column of metals on the table, soft enough to cut with a knife, reactive enough to explode in water.
Alkaline earth metal
Any element in Group 2 of the periodic table. These metals have two electrons in their outer level and are also quite reactive, though less so than alkali metals. In simple terms, Group 2 sits one column to the right of Group 1, slightly less dramatic in its reactions.
Transition metal (transition element)
Any element in Groups 3 through 12 of the periodic table. These metals can occur naturally as uncombined elements and include the iron triad and coinage metals. Think of it as: the big block in the middle of the periodic table, containing most of the familiar everyday metals (iron, copper, gold, silver).
Radioactive element
An element whose nucleus breaks down and emits particles and energy. In simple terms, the atom is unstable and slowly falls apart on its own, releasing radiation as it does so.
Metals are solids at room temperature, with one exception: mercury (Hg) is a liquid.
They are shiny (lustrous), malleable, and ductile.
Metals are good conductors of both heat and electricity.
On the periodic table, metals are located to the left of the stair-step (zigzag) line.
In a metallic bond, positively charged metal ions sit in a "sea" of delocalised electrons.
Metals give up their outer electrons easily because those electrons are not strongly held by the protons in the nucleus.
This sea of electrons explains why metals conduct electricity (electrons flow freely) and why they are malleable and ductile (layers of ions can slide over one another without breaking the bond).
When a metal bonds with a nonmetal, the metal transfers electrons to the nonmetal, forming an ionic bond.
Both atoms become ions and are more stable in that form.
Classic examples: sodium + chlorine (NaCl), lithium + fluorine (LiF).
Softer than most metals and the most reactive of all metal families.
They do not occur naturally in their elemental form because they react too readily with other elements.
Each alkali metal has one electron in its outermost energy level, which it gives up very easily.
Some elements in this family are radioactive: the nucleus breaks down and releases particles and energy.
Also very reactive and do not occur naturally in elemental form.
Each has two electrons in its outer level.
Slightly less reactive than alkali metals because it takes a bit more energy to remove two electrons than one.
The large block of metals in the centre of the periodic table.
Named "transition" metals because they sit between Group 2 and Groups 13 to 18.
Unlike alkali and alkaline earth metals, many transition metals occur in nature as uncombined (pure) elements, for example gold and platinum.
They often form coloured compounds, which is useful for identification in the lab.
Metallic bonding is the reason copper wires carry electricity through your walls: the delocalised electrons move freely from atom to atom.
Aluminium's malleability is why it can be rolled into foil thin enough to wrap food, yet its metallic bonding keeps it strong enough for aeroplane bodies.
Alkali metals are used in specialised applications: lithium in rechargeable batteries, sodium in street lights.
Transition metals show up everywhere: iron in steel construction, copper in plumbing and electronics, gold and silver in jewellery and circuitry.
Students often think all metals are hard and strong. They are not. Alkali metals (Group 1) are soft enough to cut with a butter knife.
Students sometimes assume mercury is a nonmetal because it is a liquid. Mercury is a metal; it simply has a very low melting point.
"Metallic bonding" and "ionic bonding" are sometimes confused. Metallic bonding is metal-to-metal (a sea of shared electrons). Ionic bonding is metal-to-nonmetal (electron transfer).
It is a common mistake to think transition metals are less important because they sit "in the middle." In fact, they include some of the most widely used elements on Earth (iron, copper, nickel, zinc).
⚠️ Be able to list the four defining properties of metals: shiny (lustrous), malleable, ductile, good conductor.
⚠️ Know the difference between metallic bonding (metal + metal, sea of electrons) and ionic bonding (metal + nonmetal, electron transfer).
⚠️ Know the number of outer electrons for each family: alkali metals = 1, alkaline earth metals = 2.
⚠️ Expect a question asking you to identify where metals, alkali metals, alkaline earth metals, and transition metals sit on the periodic table.
⚠️ Mercury as the exception (liquid metal at room temperature) is a favourite exam question.
True or False: All metals are solids at room temperature.
Fill in the blank: Metals that can be hammered into sheets are described as ________.
True or False: Alkali metals have two electrons in their outer energy level.
Fill in the blank: When a metal and a nonmetal bond together, they form a(n) ________ bond.
True or False: Transition metals are found in Groups 3 to 12.
Answers: 1. False (mercury is a liquid). 2. Malleable. 3. False (they have one). 4. Ionic. 5. True.
Q: What is metallic bonding, and how does it explain a metal's ability to conduct electricity?
A: Metallic bonding occurs when positively charged metal ions are surrounded by a sea of delocalised electrons. Because these electrons can move freely, they carry electrical current through the metal.
Q: Name two properties that distinguish metals from nonmetals.
A: Metals are malleable (can be hammered into sheets) and are good conductors of heat and electricity. Nonmetals are brittle and poor conductors.
Q: Why do alkali metals not occur naturally in their elemental form?
A: They are extremely reactive. With only one electron in their outer level, they readily lose it to bond with other elements, so they are always found in compounds in nature.
Q: How many outer-level electrons do alkaline earth metals have, and how does this compare to alkali metals?
A: Alkaline earth metals have two outer electrons; alkali metals have one. Both families are reactive, but alkali metals are more so because removing a single electron requires less energy.
Q: A metal and a nonmetal bond together. What type of bond is formed, and what happens to the electrons?
A: An ionic bond is formed. The metal transfers one or more electrons to the nonmetal, producing a positive ion (the metal) and a negative ion (the nonmetal) that attract each other.
This material connects directly to Chapter 17 Part 2 (Nonmetals) and Part 3 (Mixed Groups / Metalloids). Understanding how metals lose electrons is essential for grasping ionic bonding in more depth later in the course, and metallic bonding lays the groundwork for understanding conductivity in physics-adjacent units. The reactivity trends of alkali and alkaline earth metals also tie into the broader topic of periodic trends (electronegativity, ionisation energy).
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