NO!!!!
Each element has it own ground state electron configuration.
Rubidium is [Kr] 5s1
Strontium is [Kr] 5s2.
Notice that strontium has one MORE electron than Rubidium.
The symbol [Kr] is shorthand for the full electron configuration of krypton.
Both are ions and we should consider the ionic radius, not the atomic radius. Rubidium ion (Rb+) will have a larger IONIC radius than strontium ion (Sr2+). Both ions have the same electronic configuration. But strontium ion has more number of protons in the nucleus. Hence it will have greater force of attraction between the nucleus and the valence electrons, resulting in smaller size.
Cesium. For non-transition elements such as rubidium, cesium, and strontium, the most chemically similar element to any other element is always one in the same column of the Periodic Table but in an adjacent row. Since strontium is not in the same column as rubidium but cesium is in the same column and an adjacent row, the answer follows. (This rule is sometimes true also for transition elements, but not always: For example, for elements in columns 8, 9, and 10, the most nearly chemically similar element is one in the same row and an adjacent column within this group, rather than one in the same column but an adjacent row.)
The element that forms a 2+ ion with the same electronic configuration as Ar is Calcium (Ca). When Calcium loses two electrons, it attains the same electronic configuration as argon by having a full outer shell of electrons.
Options are not given in the question. But the following species will have the same electronic configuration as Br- ion: Neutral atom: Kr Cations: Rb+, Sr2+ Anion: Se2-
The electronic configuration of calcium is 1s2 2s2 2p6 3s2 3p6 4s2. In calcium hydroxide (Ca(OH)2), calcium loses its two outer electrons to form Ca2+ ion, which has the electronic configuration 1s2 2s2 2p6 3s2 3p6.
Both are ions and we should consider the ionic radius, not the atomic radius. Rubidium ion (Rb+) will have a larger IONIC radius than strontium ion (Sr2+). Both ions have the same electronic configuration. But strontium ion has more number of protons in the nucleus. Hence it will have greater force of attraction between the nucleus and the valence electrons, resulting in smaller size.
When rubidium-87 (Rb-87) converts to strontium-87 (Sr-87), it undergoes beta decay. In this process, a neutron in the rubidium nucleus is transformed into a proton, resulting in the emission of an electron, known as a beta particle, and an antineutrino. This transformation increases the atomic number from 37 (rubidium) to 38 (strontium) while the mass number remains the same at 87.
Cesium. For non-transition elements such as rubidium, cesium, and strontium, the most chemically similar element to any other element is always one in the same column of the Periodic Table but in an adjacent row. Since strontium is not in the same column as rubidium but cesium is in the same column and an adjacent row, the answer follows. (This rule is sometimes true also for transition elements, but not always: For example, for elements in columns 8, 9, and 10, the most nearly chemically similar element is one in the same row and an adjacent column within this group, rather than one in the same column but an adjacent row.)
The negative ion F has the same electronic configuration as the positive ion Ne. This is because the negative ion F gains an electron to achieve a stable octet configuration, similar to the stable electronic configuration of the noble gas Ne.
The element that forms a 2+ ion with the same electronic configuration as Ar is Calcium (Ca). When Calcium loses two electrons, it attains the same electronic configuration as argon by having a full outer shell of electrons.
Cesium(I), Cs+1 is an iso-electronic ion to Ba2+ and also iodine, I-1 ions and xenon, Xe0 atoms are iso-electronic to Ba2+ ions.They all have the [Xe] electron configuration: [2, 8, 18, 18, 8], 0
Cesium. For non-transition elements such as rubidium, cesium, and strontium, the most chemically similar element to any other element is always one in the same column of the periodic table but in an adjacent row. Since strontium is not in the same column as rubidium but cesium is in the same column and an adjacent row, the answer follows. (This rule is sometimes true also for transition elements, but not always: For example, for elements in columns 8, 9, and 10, the most nearly chemically similar element is one in the same row and an adjacent column within this group, rather than one in the same column but an adjacent row.)
Rubidium forms a +1 cation (Rb+) by losing one electron to achieve a stable electron configuration. Rubidium has one valence electron in its outermost shell, so by losing this electron, it becomes a cation.
Strontium has 38 electrons. (Protons and electrons are the same)
When the electronic configuration of any element is not the same as we expected, it is known as anomalous EC. For Eg Cromium, Copper and heavier d and f block elements.
Options are not given in the question. But the following species will have the same electronic configuration as Br- ion: Neutral atom: Kr Cations: Rb+, Sr2+ Anion: Se2-
The electronic configuration of calcium is 1s2 2s2 2p6 3s2 3p6 4s2. In calcium hydroxide (Ca(OH)2), calcium loses its two outer electrons to form Ca2+ ion, which has the electronic configuration 1s2 2s2 2p6 3s2 3p6.