Strontium Valence Electrons

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Strontium is a group 2 element - all group 2 elements have 2 valence electrons. Strontium has 36 'inner' electrons and 2 'outer' or valence electrons. 549.5, 1064.2, 4138, 5500, 6910, 8760, 10230, 11800, 15600, 17100 kJ/mol. Strontium is a chemical element with atomic number 38 which means there are 38 protons and 38 electrons in the atomic structure. The chemical symbol for Strontium is Sr. The atom consist of a small but massive nucleus surrounded by a cloud of rapidly moving electrons. The nucleus is composed of protons and neutrons. Determining Valence Electrons 1. Give the correct number of valence electrons for the element strontium, Sr, atomic #38. Which of the following electron dot notations is correct for the element calcium, Ca, atomic #20? Which of the noble gases does not have eight electrons in its outermost shell? Valence Electrons: 5s 2 Electron Dot Model. Chemical Properties of Strontium. Electrochemical Equivalent: 1.635g/amp-hr. Strontium - Sr (EnvironmentalChemistry.com)- Comprehensive information for the element Strontium - Sr is provided by this page including scores of properties, element names in many languages, most known nuclides.

Answers: 1
1.
A) sodium - 1
B) Flourine - 7
C)Boron - 3
D) Carbon - 4
2.
The element of oxygwn has 6 valence electrons.
3.
false
magnesium has 2 valance electrons but sodium has just 1.
4.
Element A is more reactive.

1) They are highly reactive.

2) They are highly reactive and are non metallic.

3) -2

4)LiCl

5) How electrons are shared

6) Each hydrogen electron has one valence electron

7) share two valence electrons

8) 85.0 g/mol

Explanation:

1) As both the kind of elements are ready to give or taken one electron, to attain noble gas configuration or full filled stability, they are highly reactive.

The element which has just one electron in valence shell will give the electron easily.

The element which has seven valence electrons will accept one electron easily.

2) Halogen have seven valence electrons. They are highly reactive as the are ready to take one electron. As they cannot give electrons they are non metals.

3) Generally oxygen can accept two electrons so its charge is '-2'

4) Formula unit is generally for ionic compound. LiCl is an ionic compound.

5) In lewis structure we write elements are then distribute electrons over all the atoms. It shows the number of bonded electrons, unshared or lone electrons as well.

6) The configuration of hydrogen is 1s1, thus it has only one valence electron/ atom.

7) In each covalent bond there are two shared electrons (shared by two atoms bonded).

8) molar mass = atomic mass of Na + Atomic mass of N + 3 X atomic mass of O

Molar mass = 23 + 14 + 3(16) = 85.0 g/mol

1. metal

2. nonmetal

3. lower

4. higher

5. in the middle

Explanation:

100% Correct of answers your welcome :)

1.metal

2.nonmetal

3.lower

4.higher

5.in the middle

Explanation:

For 1: Boron has 3 valence electrons, Carbon has 4 valence electrons, Fluorine has 7 valence electrons and Sodium has 1 valence electron.

For 2: The correct answer is 6.

For 3: The correct answer is False.

For 4: The correct answer is Element A is more reactive.

Explanation:

Valence electrons are defined as the electrons which are present in the outermost shell of an atom. The outermost shell has the highest number of principle quantum number, 'n'.

For 1:

Boron is the 5th element of the periodic table having electronic configuration of

Number of valence electrons in Boron = 2 + 1 = 3

Carbon is the 6th element of the periodic table having electronic configuration of

Number of valence electrons in carbon = 2 + 2 = 4

Fluorine is the 9th element of the periodic table having electronic configuration of

Number of valence electrons in fluorine = 2 + 5 = 7

Sodium is the 11th element of the periodic table having electronic configuration of

Number of valence electrons in sodium = 1

Hence, boron has 3 valence electrons, Carbon has 4 valence electrons, Fluorine has 7 valence electrons and Sodium has 1 valence electron.

For 2:

Oxygen is the 8th element of the periodic table having electronic configuration of

Number of valence electrons in carbon = 2 + 4 = 6

Hence, the correct answer is 6.

For 3:

Sodium is the 11th element of the periodic table having electronic configuration of

Number of valence electrons in sodium = 1

Magnesium is the 12th element of the periodic table having electronic configuration of

Number of valence electrons in magnesium = 2

Hence, the correct answer is False.

For 4:

Chemical reactivity is defined as the tendency of an element to loose of gain electrons.

We are given:

Element A has 7 valence electrons and Element B has 4 valence electrons.

Element A require 1 electron to complete its octet and Element B require 4 electrons.

So, it is easy for element A to attain 1 electron than for element B to even loose or gain 4 electrons.

Hence, the correct answer is Element A is more reactive.

D. Lithium is the least reactive element in group 1, because it is the smallest and holds its valence electron more tightly than the others in the same group.

Explanation:

Lithium is at the top of group one and has only two energy levels. It has the smallest atomic radius of all the elements in group one. This means it's valence electron is the closest one to the nucleus of all the group 1 elements. The nucleus holds this electron more tightly than other group 1 nuclei which is why lithium is the least reactive of all the group 1 metals.

Explanation:

1.Which elements had complete outer shells? Give the name and symbol for each

The elements with outer complete shells are the noble gases or inert gases or Group O elements. They are said to have a completer octet.

The elements in this group are:

Helium He Neon NeArgon ArKrypton KrXenon Xe Radon Rn

2. What do you notice about the location of the elements in #1?

The elements here are located in the last group on the periodic table and it is the p-block.

3. Which elements had only one valence electron?

The alkali metals have only one electron in their outermost shell. They are located in the first group on the periodic table. This group is made up of metals.

4. What do you notice about the location of the elements in #3?

They are located in the first group on the periodic table and they have one valence electron

5. What do you notice about the number of valence electrons as you move from left to right across a row or period in the periodic table? (Na - Mg - Al Si P S - CI - An

The number of valence electrons increases from left to right on the periodic table. Moving across a period is like going from one group to another and the number of valence electrons increases in that manner.

6. What do you notice about the number of energy levels or shells as you move down a group or column in the periodic table? (H Li - Na)

The energy levels increases. As one goes down a group the atomic radii increases as new energy levels and electronic shells are added to corresponding atoms.

7. Elements are organized into families according to their physical and chemical properties. Identify the elements that you used in Step 5 that belong to each family based on the number of valence electrons. Give the name and symbol for each element,

Group 1 or family 1 elements:

Lithium Li

Sodium Na

Potassium K

Rubidium Rb

Cesium Cs

Francium Fr

All of the elements in this group have similar chemical and physical properties. They all have one electron in their valence shell.

Alkali Metals - 1 valence electron

Alkaline Earth Metals - 2 valence electrons

Boron Family - 3 valence electrons

Carbon Family 4 valence electrons

Nitrogen Family - 5 valence electrons

Oxygen Family - 6 valence electrons

Halides - 7 valence electrons

Noble Gases - Complete outermost shell

8. What do you notice about the location of the elements in each family?

The location of each element in the family is based on the atomic numbers. This is the number of protons an atom contains.

Each element is arranged in vertical columns and they all have the same number of valence electrons.

9. How would you classify hydrogen? Why?

I will classify hydrogen as a Group O element.

Hydrogen has just one electron. This electron is located in the 1s orbital and half-filled orbitals are also stable like fully filled orbitals.

Also, hydrogen is a gas and it cannot be put into a group of metals. Therefore it would fit well into the noble gases.

10. Predict the number of valence electrons for each element based on its location in the Periodic Table of Elements. You will need to use the table in your textbook

Barium 2 electrons Alkali earth metals

Xenon 8 electrons Noble gases

Potassium 1 electron Alkali metals

Learn more:

Periodic table

Strontium valence electrons

Alkali metals

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Metals : Since metals have tendency to lose extra electrons in their valence shell and attain neutrality.

Non-metals : Since metals have tendency to gain extra electrons in their valence shell and attain neutrality.

Lower : Since lower elements can easily lose electrons from the valence shell because of weak attraction from the nucleus.

Higher : Since higher elements can not easily lose electrons from the valence shell because of strong attraction from the nucleus.

intermediate

the answers are

metal

nonmetal

lower

higher

in the middle

your picture is not part of the scientific method.

answer///carbon;

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What element has the same number valence electrons as strontium?​...

Element Strontium - Sr

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

  • Atomic Number: 38
  • Group: 2
  • Period: 5
  • Series: Alkali Earth Metals

Strontium's Name in Other Languages

  • Latin: Strontium
  • Czech: Stroncium
  • Croatian: Stroncij
  • French: Strontium
  • German: Strontium - s
  • Italian: Stronzio
  • Norwegian: Strontium
  • Portuguese: Estrôncio
  • Russian: Стронций
  • Spanish: Estroncio
  • Swedish: Strontium

Atomic Structure of Strontium

  • Atomic Radius: 2.45Å
  • Atomic Volume: 33.7cm3/mol
  • Covalent Radius: 1.91Å
  • Cross Section (Thermal Neutron Capture) σa/barns: 1.28
  • Crystal Structure: Cubic face centered
  • Electron Configuration:
    1s2 2s2p6 3s2p6d10 4s2p6 5s2
  • Electrons per Energy Level: 2,8,18,8,2
    Shell Model
  • Ionic Radius: 1.12Å
  • Filling Orbital: 5s2
  • Number of Electrons (with no charge): 38
  • Number of Neutrons (most common/stable nuclide): 50
  • Number of Protons: 38
  • Oxidation States: 2
  • Valence Electrons: 5s2
    Electron Dot Model

Chemical Properties of Strontium

  • Electrochemical Equivalent: 1.635g/amp-hr
  • Electron Work Function: 2.59eV
  • Electronegativity: 0.95 (Pauling); 0.99 (Allrod Rochow)
  • Heat of Fusion: 8.3kJ/mol
  • Incompatibilities:
  • Ionization Potential
    • First: 5.695
    • Second: 11.03
    • Third: 43.6
  • Valence Electron Potential (-eV): 25.7

Physical Properties of Strontium

  • Atomic Mass Average: 87.62
  • Boiling Point: 1657K 1384°C 2523°F
  • Coefficient of lineal thermal expansion/K-1: 23E-6
  • Conductivity
    Electrical: 0.0762 106/cm Ω
    Thermal: 0.353 W/cmK
  • Density: 2.54g/cc @ 300K
  • Description:
    Soft silvery yellow metal that will burn if ignited in air.
  • Elastic Modulus:
    • Bulk: 12/GPa
    • Rigidity: 6.03/GPa
    • Youngs: 15.7/GPa
  • Enthalpy of Atomization: 163.2 kJ/mole @ 25°C
  • Enthalpy of Fusion: 9.16 kJ/mole
  • Enthalpy of Vaporization: 150 kJ/mole
  • Flammablity Class:
  • Freezing Point:see melting point
  • Hardness Scale
    • Mohs: 1.5
  • Heat of Vaporization: 144kJ/mol
  • Melting Point: 1042K 769°C 1416°F
  • Molar Volume: 33.7 cm3/mole
  • Physical State (at 20°C & 1atm): Solid
  • Specific Heat: 0.3J/gK
  • Vapor Pressure = [email protected]°C

Regulatory / Health

  • CAS Number
    • 7440-24-6
  • 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: 0.031
    • Bone/p.p.m: 36-140
    • Liver/p.p.m: 0.05-0.36
    • Muscle/p.p.m: 0.12-0.35
    • Daily Dietary Intake: 0.8-5 mg
    • Total Mass In Avg. 70kg human: 320 mg
  • Discovery Year: 1790
  • Name Origin:
    From Strontian a small Scottish town.
  • Abundance of Strontium:
    • Earth's Crust/p.p.m.: 370
    • Seawater/p.p.m.:
      • Atlantic Suface: 7.6
      • Atlantic Deep: 7.7
      • Pacific Surface: 7.6
      • Pacific Deep: 7.7
    • Atmosphere/p.p.m.: N/A
    • Sun (Relative to H=1E12): 790
  • Sources of Strontium:
    Found in minerals celestite and strontianite. Annual world wide production is around 137,000 tons. Primary mining areas are UK, Tunisia, Russia, Germany, Mexico and USA.
  • Uses of Strontium:
    Used in flares and fireworks for crimson color. Also used in nuclear batteries in buoys and phosphorescent paint.
  • Additional Notes:
    A. Crawford first recognized strontium as an element in 1790, but it wasn't isolated until 1808 by Sir Humphry Davy in London England.

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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

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

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How Many Valence Electrons In Strontium

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Strontium Valence Electrons Count

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