The Periodic Table

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FOUNDATIONS · PERIODIC TABLE & CHEMICAL BONDING

118 elements.
One map. All of chemistry.

Every reaction you'll study for JEE or NEET — acids, batteries, drugs, alloys — comes down to how atoms arrange their outer electrons. The periodic table is the map; bonding is what happens when two locations on that map meet. Click any element to start exploring.

Click an element above to see its story.

Chapter One

The map

A period (row) tells you how many electron shells an atom has. A group (column) tells you how many electrons sit in the outermost shell — which is why elements in the same column behave alike. Click any tile below for its full profile.

Select an element from the grid to see period, group, electron configuration, and a quick fact.

Chapter Two

Trends

Three properties move in predictable directions as you scan the table. Pick one and watch Period 3 and Group 1 respond.

ACROSS PERIOD 3 (Na → Ar)

DOWN GROUP 1 (Li → K)

Chapter Three

Metal, nonmetal, or metalloid?

A jagged "staircase" line runs from Boron down to Astatine. Left of it: metals — shiny, malleable, electron-losers. Right of it: nonmetals — brittle or gaseous, electron-gainers. Sitting on the line: metalloids, with a foot in both worlds. Classify each element.

Chapter Four

Why atoms bond

Atoms bond to fill their outer shell to 8 electrons — the octet rule. How they get there decides the bond type: one atom can steal electrons (ionic), two atoms can share them (covalent), or a whole block of metal atoms can pool them into a shared "sea" (metallic). The gap in electronegativity between two atoms predicts which. Pick a pair.

Chapter Five

Drawing the bond

A Lewis structure is the octet rule drawn out in dots. Flip each card to see how the electrons actually land.

Chapter Six

Where this shows up

Ionic bonds let batteries move charge (Li⁺ ions drifting between electrodes is literally what powers your phone). Metallic bonding's "sea of electrons" is why copper wires conduct and why aluminium bends instead of shattering. Covalent bonds hold together every drug molecule, every strand of DNA, and every plastic. Metalloids like silicon — sitting exactly on the staircase — are why semiconductors, and therefore every chip in every device you own, exist at all.

Final Check

Ten questions

No pressure, no timer. Get your score, see the reasoning, retry if you want.

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Next in Chemistry Foundations — Moles, Stoichiometry & Chemical Reactions.