Calculate the effective nuclear charge of the 59th electron in Platinum using slater's rules

Please answer all questions Thanks.

18 Why did the scientist have to come up with a different atomic model after Bohr?a.    Bohr could not predict the orbitals of electrons of larger atomsb.    All of the choicesc.    Bohr assumed that electrons either emit or absorb a photon or a particle representing a quantum of    20 Which of the following /statements is/are true?I.    All ionic compounds are water-soluble.II.    Covalent compounds are mostly organic compoundsIII.    Ionic compounds are mostly inorganic compounds.  a.    I, II, IIIb.    I, IIc.    Id.    II, IIIe.    II 21 The Bohr model of the atom is known as the ______ model.

Use Slater's Rules to address these questions • What is the effective nuclear charge for the highest energy electron in F atom? • What is the effective nuclear charge for the highest energy electron in F- atom? • Which is easier to ionize (remove an electron)?

Two main-group elements are highlighted in the outline of the Periodic Table below: What can you say about these elements without knowing exactly which they are? Use that knowledge to answer the questions in the following table, if possible. Important: do not try to figure out exactly which elements are marked, and then use your knowledge of the properties of each specific element. You don't need to. You will also be marked wrong for any answer, correct or not, that can't be determined from the rough location of each marked element in the Periodic Table. Element X Element Y Which element in the gas phase is more likely to glow green or yellow in a flame? X 5 O Can't say without more information. O Element X Which element is more likely to form an ionic compound with chlorine? O Element Y O Can't say without more information. O Element X Which element in the solid state is probably brittle, so that it breaks before bending? Element Y Can't say without more information. Explanation Check

Four main-group elements a, b, c and d are highlighted in the outline of the Periodic Table below: List these elements below in order of decreasing atomic radius. For example, if an atom of a is the biggest, and b the next biggest, then your list should start b, ... a d X a с Important: don't try to figure out exactly which elements are marked, and then use your knowledge of the properties of each specific element. You don't need to. You will also be marked wrong for any answer, correct or not, that can't be determined from only the rough location of each marked element in the Periodic Table. 0.000 b S

According to Coulomb's Law... O The energy between two oppositely charged particles decreases as the distance between them decreases. O The energy between two like charged particles increases as the distance between them increases. O The energy between two like charged particles decreases as the distance between them decreases. O The energy between two oppositely charged particles decreases as the distance between them increases.

How did DeBroglie’s idea of matter waves rationalize the Bohr model of the atom? A.  It showed that Bohr’s orbits were similar to planetary orbits. B.  It showed that Bohr’s orbits were areas of constructive interference, with the space between showing destructive interference. C.  It showed that Bohr’s orbits were a result of the photoelectric effect. D.  It showed that Bohr’s orbits obeyed the uncertainty principle. E.  None of the above are true.

Quantum mechanics

Imagine a universe where there are three spin states for the electron instead of two (for example, spin up, spin down, and spin cray-cray). The number of subshells per shell and number of orbitals per subshell stay the same, but an orbital now holds three electrons instead of two. The names of the elements stay the same. Draw the top three rows of what this new periodic table would look like, indicating which elements are in which groups in our new universe, and show the electron configurations of each of the elements of these three rows.