📈 Property Trends

Visualize how element properties change across the periodic table. Select a property and optionally filter by period.

Tendency to attract electrons in a chemical bond

Electronegativity by Atomic Number

← Lower atomic numberHigher atomic number →

#	Symbol	Name	Electronegativity (Pauling)	Category
9	F	Fluorine	3.98	Halogen
8	O	Oxygen	3.44	Nonmetal
17	Cl	Chlorine	3.16	Halogen
7	N	Nitrogen	3.04	Nonmetal
36	Kr	Krypton	3	Noble gas
35	Br	Bromine	2.96	Halogen
53	I	Iodine	2.66	Halogen
54	Xe	Xenon	2.6	Noble gas
16	S	Sulfur	2.58	Nonmetal
6	C	Carbon	2.55	Nonmetal
34	Se	Selenium	2.55	Nonmetal
79	Au	Gold	2.54	Transition metal
74	W	Tungsten	2.36	Transition metal
82	Pb	Lead	2.33	Post-transition metal
45	Rh	Rhodium	2.28	Transition metal
78	Pt	Platinum	2.28	Transition metal
1	H	Hydrogen	2.2	Nonmetal
44	Ru	Ruthenium	2.2	Transition metal
46	Pd	Palladium	2.2	Transition metal
76	Os	Osmium	2.2	Transition metal
77	Ir	Iridium	2.2	Transition metal
85	At	Astatine	2.2	Halogen
15	P	Phosphorus	2.19	Nonmetal
33	As	Arsenic	2.18	Metalloid
42	Mo	Molybdenum	2.16	Transition metal
52	Te	Tellurium	2.1	Metalloid
51	Sb	Antimony	2.05	Metalloid
5	B	Boron	2.04	Metalloid
83	Bi	Bismuth	2.02	Post-transition metal
32	Ge	Germanium	2.01	Metalloid

Periodic trends are patterns in element properties that arise from the periodic table's arrangement by atomic number. Key trends include:

Electronegativity generally increases across a period (left to right) and decreases down a group.
Atomic radius decreases across a period and increases down a group.
Ionization energy increases across a period and decreases down a group.
Electron affinity becomes more negative across a period for most elements.

These trends are explained by changes in nuclear charge, electron shielding, and the distance of valence electrons from the nucleus.