Cesium Valence Electrons

Element Cesium - Cs

1. Cesium Valence Electrons Ion
2. Cesium Number Of Valence Electrons
3. Cesium Electron Configuration
4. Cesium Valence Electron Configuration
5. How Many Valence Electrons In Cs

Complete and detailed technical data about the element Cesium in the Periodic Table. Click here to buy a book, photographic periodic table poster, card deck, or 3D print based on the images you see here! There is 1 valence electrons in caesium. If you look at a periodic table, it is in the first group. This means that since it is in the first group it has 1 valence electron. If you go all of the.

Comprehensive data on the chemical element Cesium is provided on this page; including scores of properties, element names in many languages, most known nuclides of Cesium. 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.

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Overview of Cesium

• Atomic Number: 55
• Group: 1
• Period: 6
• Series: Alkali Metals

Cesium's Name in Other Languages

• Latin: Caesium
• Czech: Cesium
• Croatian: Cezij
• French: Césium
• German: Zäsium - s
• Italian: Cesio
• Norwegian: Cesium
• Portuguese: Césio
• Russian: Цеэий
• Spanish: Cesio
• Swedish: Cesium

Atomic Structure of Cesium

• Atomic Radius: 3.34Å
• Atomic Volume: 71.07cm³/mol
• Covalent Radius: 2.35Å
• Cross Section (Thermal Neutron Capture)σ_a/barns: 29
• Crystal Structure: Cubic body centered
• Electron Configuration:

  1s² 2s²p⁶ 3s²p⁶d¹⁰ 4s²p⁶d¹⁰ 5s²p⁶ 6s¹

• Electrons per Energy Level: 2,8,18,18,8,1

  Shell Model
  

• Ionic Radius: 1.67Å
• Filling Orbital: 6s¹
• Number of Electrons (with no charge): 55
• Number of Neutrons (most common/stable nuclide): 78
• Number of Protons: 55
• Oxidation States: 1
• Valence Electrons: 6s¹

  Electron Dot Model
  

Cesium Valence Electrons Ion

Chemical Properties of Cesium

• Electrochemical Equivalent: 4.9587g/amp-hr
• Electron Work Function: 2.14eV
• Electronegativity: 0.79 (Pauling); 0.86 (Allrod Rochow)
• Heat of Fusion: 2.092kJ/mol
• Incompatibilities:
• Ionization Potential
  • First: 3.894
  • Second: 25.1
• Valence Electron Potential (-eV): 8.62

Physical Properties of Cesium

• Atomic Mass Average: 132.9054
• Boiling Point: 944K 671°C 1240°F
• Coefficient of lineal thermal expansion/K^-1: 97E^-6
• Conductivity

  Electrical: 0.0489 10⁶/cm Ω
  Thermal: 0.359 W/cmK

• Density: 1.873g/cc @ 300K
• Description:

  Soft light silvery-white alkali metal.

• Elastic Modulus:
  • Bulk: 1.6/GPa
  • Rigidity: 0.65/GPa
  • Youngs: 1.7/GPa
• Enthalpy of Atomization: 78.2 kJ/mole @ 25°C
• Enthalpy of Fusion: 2.1 kJ/mole
• Enthalpy of Vaporization: 65.9 kJ/mole
• Flammablity Class:
• Freezing Point:see melting point
• Hardness Scale
  • Brinell: 0.14 MN m^-2
  • Mohs: 0.2
• Heat of Vaporization: 67.74kJ/mol
• Melting Point: 301.7K 28.55°C 83.39°F
• Molar Volume: 70.73 cm³/mole
• Physical State (at 20°C & 1atm): Solid
• Specific Heat: 0.24J/gK
• Vapor Pressure 2.5kPa

Regulatory / Health

• CAS Number
  • 7440-46-2
• RTECS: FK9225000
• 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: 0.0038
  • Bone/p.p.m: 0.013-0.052
  • Liver/p.p.m: 0.04-0.05
  • Muscle/p.p.m: 0.07-1.6
  • Daily Dietary Intake: 0.004-0.03 mg
  • Total Mass In Avg. 70kg human: 6 mg

Who / Where / When / How

• Discoverer: Gustov R. Kirchoff, Robert Bunsen
• Discovery Location: Heidelberg Germany
• Discovery Year: 1860
• Name Origin:

  Latin: caesius (sky blue); its salts turn flames blue.

• Abundance of Cesium:
  • Earth's Crust/p.p.m.: 3
  • Seawater/p.p.m.: 0.0003
  • Atmosphere/p.p.m.: N/A
  • Sun (Relative to H=1E¹²): 80
• Sources of Cesium:

  Found in pollucite [(Cs₄Al₄Si₉O_{26).H2O] and as trace in lepidolite. World production is around 20 tons per year. Primary mining areas are in Bernic Lake (Manitoba, Canada), Bikita (Zimbabwe) and South-West Africa.}

• Uses of Cesium:

  Used as a 'getter' to remove air traces in vacuum tubes. Since it ionizes readily, it is used as an ion rocket motor propellant. Also used in photoelectric cells, atomic clocks, infared lamps.

• Additional Notes:

  Cesium can have very serious effects on the body if taken in excess.

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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.

Related Resources

• Anatomy of the Atom
  Answers many questions regarding the structure of atoms.
• Molarity, Molality and Normality
  Introduces stoichiometry and explains the differences between molarity, molality and normality.
• Molar Mass Calculations and Javascript Calculator
  Molar mass calculations are explained and there is a JavaScript calculator to aid calculations.
• Chemical Database
  This database focuses on the most common chemical compounds used in the home and industry.

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As mentioned above, the characteristic chemical property of a metalatom is to lose one or more of its electrons to form a positive ion. However, certain metals lose electrons much more readily than others. In particular, cesium (Cs) can give up its valence electron more easily than can lithium (Li). In fact, for the alkali metals (the elements in Group 1), the ease of giving up an electron varies as follows: Cs > Rb > K > Na > Li with Cs the most likely, and Li the least likely, to lose an electron. In going down the group, the metals become more likely to lose an electron because the electron being removed lies increasingly farther from the positive nucleus. That is, the electron lost from Cs to form Cs⁺ lies at a much greater distance from the attractive positive nucleus—and is thus easier to remove—than the electron that must be removed from a lithium atom to form Li⁺. The same trend also is seen among the Group 2 elements (the alkaline-earth metals); the farther down in the group the metal resides, the more likely it is to lose an electron.

Cesium Number Of Valence Electrons

Just as metals vary somewhat in their properties, so do nonmetals. As a general rule, the most chemically active metals appear in the lower left-hand region of the periodic table, whereas the most chemically active nonmetals appear in the upper right-hand region. The properties of the semimetals, or metalloids, lie between those of the metals and the nonmetals.

The ionization energy of an element is the energy required to remove an electron from an individual atom. Here M(g) represents a metal in the vapour state.

Cesium Electron Configuration

Metal atoms lose electrons to nonmetal atoms because metals typically have relatively low ionization energies. Metals at the bottom of a group lose electrons more easily than those at the top. That is, ionization energies tend to decrease in going from the top to the bottom of a group. Nonmetals, which are found in the right-hand region of the periodic table, have relatively large ionization energies and therefore tend to gain electrons. Ionization energies generally increase in going from left to right across a given period. Thus, the elements that appear in the lower left-hand region of the periodic table have the lowest ionization energies (and are therefore the most chemically active metals), while the elements that occur in the upper right-hand region of the periodic table have the highest ionization energies (and are thus the most chemically active nonmetals).

As mentioned above, when a nonmetallic element reacts with a metallic element, electrons are transferred from the atoms of the metal to the atoms of the nonmetal, forming positive ions (cations) and negative ions (anions), respectively. This produces an ionic compound. For example, lithium and fluorine (F) react to form lithium fluoride (LiF), which contains Li⁺ and F⁻ ions.

In contrast, when two nonmetallic elements react, the atoms combine to form molecules by sharing electrons. Bonds formed by electron sharing between atoms are called covalent bonds. The electrons are shared rather than transferred, because the two nonmetal atoms have comparable attractive powers for the electrons in the bond. For example, fluorinegas consists of F₂ molecules in which the fluorine atoms are bound together by sharing a pair of electrons, one contributed by each atom. In addition, hydrogen and fluorine react to form hydrogen fluoride, which contains HF molecules. The hydrogen and fluorine atoms are bound together by a pair of electrons, one electron contributed by the hydrogen atom and one by the fluorine atom. Although the electrons are shared between the hydrogen and the fluorine atoms, in this case they are not shared equally. This is clear from the fact that the HF molecule is polar; the hydrogen atom has a partial positive charge (δ+), while the fluorine atom has a partial negative charge (δ−): H―F
δ+ δ− (In this example the symbol δ stands for a number less than one.) This electrical polarity occurs because the shared electrons spend more time close to the fluorine atom than to the hydrogen atom. That is, fluorine has greater affinity for the shared electrons than does hydrogen. This leads to a polar covalent bond.

Cesium Valence Electron Configuration

The ability of an atom to attract the electrons shared with another atom is termed its electronegativity. The relative electronegativities of the various atoms can be determined by measuring the polarities of the bonds involving the atoms in question. Fluorine has the greatest electronegativity value (4.0, according to the Pauling scale), and cesium and francium have the smallest values (0.79 and 0.7, respectively). In general, nonmetal atoms have higher electronegativities than metal atoms. In the periodic table, electronegativity typically increases in moving across a period and decreases in going down a group. When elements with very different electronegativities (such as fluorine and cesium) react, one or more electrons are transferred to form an ionic compound. For example, cesium and fluorine react to form CsF, which contains Cs⁺ and F⁻ ions. When nonmetal atoms with differing electronegativities react, they form molecules with polar covalent bonds.

How Many Valence Electrons In Cs

Another important atomic property is atomic size. The sizes of atoms vary; atoms generally tend to become larger in going down a group on the periodic table and smaller in going from left to right across a period.