Lithium Valence Electrons

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The number of electrons in each element’s electron shells, particularly the outermost valence shell, is the primary factor in determining its chemical bonding behavior. In the periodic table, the elements are listed in order of increasing atomic number Z. Electron configuration of Lithium is He 2s1. Possible oxidation states are +1. Lithium has a single electron in the second principal energy level and so we say that lithium has one valence electron. Beryllium has two valence electrons. How many valence electrons does boron have? You must recognize that the second principal energy level consists of both the 2 s and the 2 p sublevels and so the answer is three.

Electron Configuration

The electrons in an atom fill up its atomic orbitals according to the Aufbau Principle; 'Aufbau,' in German, means 'building up.' The Aufbau Principle, which incorporates the Pauli Exclusion Principle and Hund's Rule prescribes a few simple rules to determine the order in which electrons fill atomic orbitals:

  1. Electrons always fill orbitals of lower energy first. 1s is filled before 2s, and 2s before 2p.
  2. The Pauli Exclusion Principle states no two electrons within a particular atom can have identical quantum numbers. In function, this principle means that if two electrons occupy the same orbital, they must have opposite spin.
  3. Hund's Rule states that when an electron joins an atom and has to choose between two or more orbitals of the same energy, the electron will prefer to enter an empty orbital rather than one already occupied. As more electrons are added to the atom, these electrons tend to half-fill orbitals of the same energy before pairing with existing electrons to fill orbitals.

Valency and Valence Electrons

The outermost orbital shell of an atom is called its valence shell, and the electrons in the valence shell are valence electrons. Valence electrons are the highest energy electrons in an atom and are therefore the most reactive. While inner electrons (those not in the valence shell) typically don't participate in chemical bonding and reactions, valence electrons can be gained, lost, or shared to form chemical bonds. For this reason, elements with the same number of valence electrons tend to have similar chemical properties, since they tend to gain, lose, or share valence electrons in the same way. The Periodic Table was designed with this feature in mind. Each element has a number of valence electrons equal to its group number on the Periodic Table. This table illustrates a number of interesting, and complicating, features of electron configuration.

First, as electrons become higher in energy, a shift takes place. Up until now, we have said that as the principle quantum number, increases, so does the energy level of the orbital. And, as we stated above in the Aufbau principle, electrons fill lower energy orbitals before filling higher energy orbitals. However, the diagram above clearly shows that the 4s orbital is filled before the 3d orbital. In other words, once we get to principle quantum number 3, the highest subshells of the lower quantum numbers eclipse in energy the lowest subshells of higher quantum numbers: 3d is of higher energy than 4s.

Second, the above indicates a method of describing an element according to its electron configuration. As you move from left to right across the periodic table, the above diagram shows the order in which orbitals are filled. If we were the actually break down the above diagram into groups rather than the blocks we have, it would show how exactly how many electrons each element has. For example, the element of hydrogen, located in the uppermost left-hand corner of the periodic table, is described as 1s1, with the s describing which orbital contains electrons and the 1 describing how many electrons reside in that orbital. Lithium, which resides on the periodic table just below hydrogen, would be described as 1s22s1. The electron configurations of the first ten elements are shown below (note that the valence electrons are the electron in highest energy shell, not just the electrons in the highest energy subshell).

The Octet Rule

Our discussion of valence electron configurations leads us to one of the cardinal tenets of chemical bonding, the octet rule. The octet rule states that atoms becomeespecially stable when their valence shells gain a full complement of valence electrons. For example, in above, Helium (He) and Neon (Ne) have outer valence shells that are completely filled, so neither has a tendency to gain or lose electrons. Therefore, Helium and Neon, two of the so-called Noble gases, exist in free atomic form and do not usually form chemical bonds with other atoms.

Valence Electrons Calculator

Most elements, however, do not have a full outer shell and are too unstable to exist as free atoms. Instead they seek to fill their outer electron shells by forming chemical bonds with other atoms and thereby attain Noble Gas configuration. An element will tend to take the shortest path to achieving Noble Gas configuration, whether that means gaining or losing one electron. For example, sodium (Na), which has a single electron in its outer 3s orbital, can lose that electron to attain the electron configuration of neon. Chlorine, with seven valence electrons, can gain one electron to attain the configuration of argon. When two different elements have the same electron configuration, they are called isoelectronic.

Lithium Valence Electrons

Diamagnetism and Paramagnetism

The electron configuration of an atom also has consequences on its behavior in relation to magnetic fields. Such behavior is dependent on the number of electrons an atom has that are spin paired. Remember that Hund's Rule and the Pauli Exclusion Principle combine to dictate that an atom's orbitals will all half-fill before beginning to completely fill, and that when they completely fill with two electrons, those two electrons will have opposite spins.

An atom with all of its orbitals filled, and therefore all of its electrons paired with an electron of opposite spin, will be very little affected by magnetic fields. Such atoms are called diagmetic. Conversely, paramagnetic atoms do not have all of their electrons spin-paired and are affected by magnetic fields. There are degrees of paramagnetism, since an atom might have one unpaired electron, or it might have four.

Element Lithium - Li

Lithium Valence Electrons Atoms

Comprehensive data on the chemical element Lithium is provided on this page; including scores of properties, element names in many languages, most known nuclides of Lithium. Common chemical compounds are also provided for many elements. In addition technical terms are linked to their definitions and the menu contains links to related articles that are a great aid in one's studies.

Lithium Menu

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Overview of Lithium

Lithium Valence Electrons Element

  • Atomic Number: 3
  • Group: 1
  • Period: 2
  • Series: Alkali Metals

Lithium's Name in Other Languages

  • Latin: Lithium
  • Czech: Lithium
  • Croatian: Litij
  • French: Lithium
  • German: Lithium - s
  • Italian: Litio
  • Norwegian: Litium
  • Portuguese: Litio
  • Russian: Литий
  • Spanish: Lítio
  • Swedish: Litium

Atomic Structure of Lithium

  • Atomic Radius: 2.05Å
  • Atomic Volume: 13.1cm3/mol
  • Covalent Radius: 1.23Å
  • Cross Section (Thermal Neutron Capture) σa/barns: 70.5
  • Crystal Structure: Cubic body centered
  • Electron Configuration:
    1s2 2s1
  • Electrons per Energy Level: 2,1
    Shell Model
  • Ionic Radius: 0.76Å
  • Filling Orbital: 2s1
  • Number of Electrons (with no charge): 3
  • Number of Neutrons (most common/stable nuclide): 4
  • Number of Protons: 3
  • Oxidation States: 1
  • Valence Electrons: 2s1
    Electron Dot Model
Lithium valence electrons

Chemical Properties of Lithium

  • Electrochemical Equivalent: 0.259g/amp-hr
  • Electron Work Function: 2.9eV
  • Electronegativity: 0.98 (Pauling); 0.97 (Allrod Rochow)
  • Heat of Fusion: 3kJ/mol
  • Incompatibilities:
    water, acids, oxidizing agents
  • Ionization Potential
    • First: 5.392
    • Second: 76.638
    • Third: 122.451
  • Valence Electron Potential (-eV): 19

Physical Properties of Lithium

  • Atomic Mass Average: 6.941
  • Boiling Point: 1615.15K 1342°C 2448°F
  • Coefficient of lineal thermal expansion/K-1: 56E-6
  • Conductivity
    Electrical: 0.108 106/cm Ω
    Thermal: 0.847 W/cmK
  • Density: 0.534g/cc @ 300K
  • Description:
    Soft silvery-white metal. Lightest of metals.
  • Elastic Modulus:
    • Bulk: 11/GPa
    • Rigidity: 4.24/GPa
    • Youngs: 4.91/GPa
  • Enthalpy of Atomization: 160.7 kJ/mole @ 25°C
  • Enthalpy of Fusion: 3 kJ/mole
  • Enthalpy of Vaporization: 134.7 kJ/mole
  • Flammablity Class: Flammable solid
  • Freezing Point:see melting point
  • Hardness Scale
    • Mohs: 0.6
  • Heat of Vaporization: 145.92kJ/mol
  • Melting Point: 453.85K 180.7°C 357.3°F
  • Molar Volume: 13 cm3/mole
  • Physical State (at 20°C & 1atm): Solid
  • Specific Heat: 3.6J/gK
  • Vapor Pressure = 1.63E-08Pa@180.7°C

Regulatory / Health

  • CAS Number
    • 7439-93-2
  • UN/NA ID and ERG Guide Number
    • UN1415 / 138
  • RTECS: OJ5540000
  • OSHAPermissible Exposure Limit (PEL)
    • No limits set by OSHA
  • OSHA PEL Vacated 1989
    • No limits set by OSHA
  • NIOSHRecommended Exposure Limit (REL)
    • No limits set by NIOSH
  • Levels In Humans:
    Note: this data represents naturally occuring levels of elements in the typical human, it DOES NOT represent recommended daily allowances.
    • Blood/mg dm-3: 0.004
    • Bone/p.p.m: 1.3
    • Liver/p.p.m: 0.025
    • Muscle/p.p.m: 0.023
    • Daily Dietary Intake: 0.1-2 mg
    • Total Mass In Avg. 70kg human: 7 mg
Lithium Valence Electrons

Who / Where / When / How

  • Discoverer: Johann A. Arfvedson
  • Discovery Location: Stockholm Sweden
  • Discovery Year: 1817
  • Name Origin:
    Greek: lithos (stone)
  • Abundance of Lithium:
    • Earth's Crust/p.p.m.: 20
    • Seawater/p.p.m.: 0.17
    • Atmosphere/p.p.m.: N/A
    • Sun (Relative to H=1E12): 10
  • Sources of Lithium:
    Spodumene, ambylgonite, lepidolite and desert lake brines. Also obtained by passing electric charge through melted lithium chloride. Around 39,000 tons of lithium is produced each year. The primary source of lithium is the USA.
  • Uses of Lithium:
    Used in batteries, ceramics, glass, lubricants, alloy hardeners, pharmaceuticals, hydrogenating agents, heat transfer liquids, rocket propellants, vitamin A synthesis, nuclear reactor coolant, underwater buoyancy devices and the production of tritium. Deoxidizer in copper and copper alloys.
  • Additional Notes:
    Lithium was first isolated in 1821 by W.T Brande. Near its melting point, lithium ignites in air. Lithium posses a dangerous fire and explosion risk when exposed to water, acids or oxidizing agents. It reacts exothermally with nitrogen in moist air at high temperatures. In solution lithium is toxic and targets the central nervous system.
Lithium fluoride valence electrons

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References

A list of reference sources used to compile the data provided on our periodic table of elements can be found on the main periodic table page.

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    This database focuses on the most common chemical compounds used in the home and industry.

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Lithium Valence Electrons

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