Give examples of what isoelectronic species is.
The species with the same electronic configuration are said to be isoelectronic.All isoelectronic species have the same electronic configuration.
All isoelectronic species have the same electronic configuration.
The species must have the same number of electrons.He, H, and Li+ are all isoelectronic species and have the same name.
He, H, and Li+ are all isoelectronic species and have the same name.
Write the electronic configuration for the neutral2 atoms of the elements to decide if two or more species are isoelectronic.Attach electrons to the atom's highest energy level if two or more are added.
If you want to remove electrons from the atom's highest energy level, write the electronic configuration of any ion.
Add electrons to the atom's highest occupied energy level.
Two or more species are said to be isoelectronic if they have the same electronic configuration.
The isoelectronic species have similar chemical properties.The Noble Gas helium: 1s2 has the same ground-state electronic configuration as the other isoelectronic species.
Consider an atom of the element Ar.The number 18 is the atomic number of Argon.An atom of argon has 18 positively charged protons in its nucleus and 18 negatively charged electrons "orbiting" the nucleus in the various energy levels.
The only element with a ground-state electronic configuration is Argon.
There are elements that can have a ground-state electronic configuration.
Consider an atom of chlorine.The number 17 is the atomic number of chlorine.An atom of chlorine has 17 positively charged protons in its nucleus and 17 negatively charged electrons "orbiting" the nucleus in various energy levels.
Like all Group 17 elements, chlorine atoms can form an anion with a charge of 1-.
If the chlorine atom gains an electron, it will form the chloride ion.
Where will this electron go?This energy level will be completed when it enters the 3p subshell.
chlorine atom + electron chloride ion
The electronic configuration of the ion is 1s22p63s23p6.The electronic configuration of an atom in the ground-state is also 1s22p63s23p6.The isoelectronic nature of the chloride ion is stated by us.
It is possible for cations to be isoelectronic with the argon atom in its ground state.
An atom of K is in its ground state.The number 19 is the atomic number of the substance.The nucleus of an atom has 19 positively charged protons.There are 19 negatively charged electrons in the nucleus of a potassium atom.The first energy level is 2 electrons in the s subshell and the second and third levels are 6 and 2 electron respectively.
Like all Group 1 elements, potassium will lose an electron to form a cation.
K+ + e-configuration electron 1s22p63s23p64s1
The electronic configuration of the potassium ion, K+, is the same as that of an atom of argon, Ar.Ar, Cl-, and K+ are said to be isoelectronic species.
Like all Group 2 metals, calcium will lose 2 electrons from its highest energy.The electronic configuration for Ca2+ is said to be Ar, Cl- and K+.
The first 20 elements of the Periodic Table are isoelectronic with atoms of a Group 18 (Noble Gas) element.
1s22p63p6 isoelectronic with Ne and anions.
Which species is not isoelectronic with Al3+?Justify your answer.
What is the question asking you to do?Determine which species is not isoelectronic.Justify your answer.
Determine which species is not isoelectronic.Justify your answer.
What data have you been given?The data is from the question: Formula of the species.
What is the relationship between your knowledge and what you need to know?The isoelectronic species have the same electronic configuration.Write the electronic configuration of the species: Al, Z, and 1s22p63s23p1 Atom of Al loses 3 electrons from the highest energy level to form Al3+.
The atom of Al loses 3 electrons from the highest energy level to form Al3+.
The atom of Na loses 1 electron from the highest energy level to form Na+.
The atom of O gains 2 electrons to form O2.
The atom of B loses 3 electrons from the second energy level to form B3+.
Al3+, Na+ and O2 all have the same electronic configuration, so decide which one is not isoelectronic.B3+ is not isoelectonic with Al3+.
All of the species have the same electronic configuration.B3+ is not isoelectonic with Al3+.
Is your answer believable?Al3+, Na+, and O2 all have the same number of electrons, but B3+ has a different number.No.13 - 3 is 10 no.11 - 1 is 10 no.Z(O) + 8 + 2 equals 10 no.B3+ can't be isoelectronic with the other species because they all have 10 electrons in total.
Al3+, Na+, and O2 all have the same number of electrons, but B3+ has a different number.No.13 - 3 is 10 no.11 - 1 is 10 no.Z(O) + 8 + 2 equals 10 no.Z(B) -3 is 5, 3 and 2.
B3+ can't be isoelectronic with the other species because they have 10 electrons in total.
The solution to the problem "species that is not isoelectronic and justify answer" is the electronic configuration of B3+ (1s2).
The electronic configuration of B3+ is not the same as the electronic one of Al3+.
1.For the purposes of this discussion, we will assume all species are in their ground-state electronic configuration.
2."neutral" means neither positively nor negatively charged.The term neutral can be used to mean neither acidic nor basic.
3.The term "orbiting" is being used to describe the motion of electrons around the nucleus, but should not be taken literally.