Silver (Ag)
Silver conducts electricity and heat better than any other element.
Silver properties
- Atomic mass
- 107.87 u
- Category
- Transition metal
- Group
- 11
- Period
- 5
- Block
- d-block
- State at room temp.
- Solid
- Electronegativity
- 1.93
- Melting point
- 1,234.93 K (961.8 °C)
- Boiling point
- 2,435 K (2,161.8 °C)
- Density
- 10.49 g/cm³
- Atomic radius
- 172 pm
- Ionization energy
- 7.576 eV
- Electron affinity
- 1.302 eV
- Radioactive
- No, has stable isotopes
- Discovered
- Ancient
Silver electron configuration
- Electron configuration
- [Kr] 4d10 5s1
- Full electron configuration
- 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s1
- Electron shells
- 2 · 8 · 18 · 18 · 1
The electron configuration of Silver (Ag) is [Kr] 4d10 5s1. Its 47 electrons are arranged in shells as 2, 8, 18, 18, 1.
Protons, neutrons and electrons in Silver
A neutral Silver atom has 47 protons and 47 electrons. Most Silver atoms have about 61 neutrons: the atomic mass rounded to 108, minus the atomic number 47.
Neutrons are approximate: atoms of the same element can have different numbers of neutrons (isotopes). Atomic number and mass
How many valence electrons does Silver have?
1
Silver has 1 valence electron, counting the electrons in its outermost s subshell. Like most transition metals, it can also use d electrons in bonding.
Silver orbital diagram
Each box is an orbital that holds up to two electrons with opposite spins (↑↓). The inner shells are the same as the noble gas in brackets. How to write electron configurations
Molar mass of Silver
107.87 g/mol
One mole of Silver atoms (6.022 × 10²³ atoms) has a mass of 107.87 grams. Use this value to convert between grams and moles.
Compounds containing Silver
Silver facts
- Silver conducts electricity and heat better than any other element.
- Silver ions are toxic to many bacteria, so silver is used in some wound dressings.
- Silver (Ag) has atomic number 47 and is a solid at room temperature. It has been known since ancient times.
Position in the periodic table
Silver is element 47, in period 5 and group 11 of the periodic table, in the d-block.
Uses of Silver
Silver is used in jewelry, tableware, coins, and investment bars, but about half of all silver now goes into industrial uses. It is used in electrical contacts and switches and in the conductive paste printed on most solar cells. Silver is also used in brazing alloys, mirrors, and silver-oxide button batteries, and traditionally in the light-sensitive silver halides of photographic film.
Who discovered Silver?
Silver has been known since ancient times and has been mined and worked into ornaments, tableware, and coins for thousands of years. Its symbol, Ag, comes from the Latin word argentum.
Where does the name come from?
Silver comes from the Old English seolfor, a word shared with other Germanic languages whose earlier origin is unclear. The symbol Ag comes from the Latin argentum, from an ancient root meaning 'shining' or 'white'.
Same group
Compare Silver
FAQ
What is the electron configuration of Silver?
The electron configuration of Silver (Ag) is [Kr] 4d10 5s1. Its 47 electrons are arranged in shells as 2, 8, 18, 18, 1.
How many protons, neutrons and electrons does Silver have?
A neutral Silver atom has 47 protons and 47 electrons. Most Silver atoms have about 61 neutrons: the atomic mass rounded to 108, minus the atomic number 47.
How many valence electrons does Silver have?
Silver has 1 valence electron, counting the electrons in its outermost s subshell. Like most transition metals, it can also use d electrons in bonding.
What is the molar mass of Silver?
The molar mass of Silver is 107.87 g/mol. This is the same number as its atomic mass, 107.87 u.
Is Silver a metal?
Yes. Silver is a transition metal, so it is a metal.
Is Silver radioactive?
Ordinary Silver is not radioactive: it has at least one stable isotope. Like every element, it also has radioactive isotopes, most of them made in laboratories.
Where is Silver on the periodic table?
Silver is element 47, in period 5 and group 11 of the periodic table, in the d-block.