a) If we move from top to bottom along a group, size of atoms, anions and cations increases as energy levels increases with increasing number of electrons.
While across a period from left to right the atom and ions size decreases as number of electrons increasing in the same energy levels so nucleons attract more the electrons and decrease the size.
b) Ionization energy is the minimum energy required to remove an outermost electron from electronic shell. Along a group from top to bottom it decreases as size of elements increasing so attraction of outermost electrons towards nucleons is decreasing.
Whereas boundation of electrons towards nucleon across the period from left to right is increasing. So the energy required to remove an electron is going to be difficult from left to right.
c) Electron affinity is the energy released when we add an electron to the outermost shell of the atom. Electron affinity along a group decreases and across the period increases. Down the group electrons are farther away from the nucleus. So it will have very less tendency to accept any external electrons. Across a period the elements have tendency to gain the octet stability so after adding an electron it gets extra octet stability and it has more electron attraction power.
d) Electronegativity is the tendency to attract an electron towards an atom. Its trend is similar to ionisation energy trend. Along the period increases while across the group decreases. It is because across the period electron density increases. The number of energy sub shells are same but number of electrons are increasing so the electronegativity increases.
Along the group, the number of sub shell is increasing so the distance between the nucleons and electrons is increasing and attraction decreasing so the electronegativity decreases.
12. Give the general trend in the periodic table (period, group) for the main group elements...
7. Which element has the following electron configurations? lon: [Ar]3d10 lon (-1 charge): [Kr]5s4d105p6 8. Write the following in order of increasing size As O Br Br Na Rb Te²- F- 02- 9. Arrange these elements in order of decreasing first ionization energy: CI, S, Sn, Pb 10. Choose the element with a more negative (exothermic) electron affinity in each pair: K or Cs Si or P Ga or Br Mg or s 11. a) Which has a higher ionization...
- Class period! Unit 4: Periodic Trends "lonization Energy Trend" - Wksh # 4 2 Directions: Please answer each fill in the blank with the best answer. 1. The energy required to remove an electron from a gaseous atom is called the T ilas_energy. 2. When an electron is removed the atom gets a 3. The energy required to remove a second electrons is called the charge. energy. 4. It always requirest i -- to remove a second electron. 5....
What is the general trend in electronigativity within a group of elements in the periodic table?
For the main group elements,in general, upon going from left to right across a period of the periodic table, the ionization energy__,theatomicsize,__ and the metallic character__
Explain why the effective nuclear charge increases across a row for the main group elements, but is nearly constant across a period in the transition metals. Explain why transition metals do not show the same strong trend in atomic radius as the main group elements (and even start to get larger across the row). Explain why the ionization energies of the transition metals are very similar to each other and do not follow the same trends as the main group...
Periodic Trends in Group
II
Objective
In this experiment, the trend in one of the several periodic
properties for group II of the Periodic Table will be
determined.
Introduction
Elements in the same group of the Periodic Table have similar
chemical and physical properties that gradually change as one goes
from one element in the group to the next. By observing the trends
in properties, the elements can be arranged in the order in which
they appear in the Periodic...
A) As B) Sb C) P D)Bi E)N 10. In which of the series of elements listed below would the elements have most nearly the same atomic radius? A) Na, K. Rb, Cs B)F, CI, Br.I C) Na, Mg. Al, Si D) Sc, Ti, V, Cr E)B, Si, As, Te Which of the following properties, in general, increases from left to right across a period in the periodic table? A) ionic charge 11、 B) atomic radius C) density D) ionization...
What is the general trend in ionization energy across a row on the periodic table? Using a ground state electron configuration as your basis of comparison, explain Why the ionization energy of boron is less than that of beryllium Why the ionization energy of oxygen is less than that of nitrogen
State where in the periodic table these elements appear: Part A elements with the valence-shell electron configuration ns2np5 Part B elements that have three unpaired p electrons Part C an element whose valence electrons are 4s24p1 Express your answer as the group and period number separated by a comma. Part D the d-block elements: groups 3-8, groups 3-12, groups 1-2, Lanthanides, or Actinides
Using the attached sheet, find where each element is located
on this new periodic table.
Period-> Moun is 16 HS hydrogen He 4.C02802 boron riges oxyge fuoring 1.00794 thlum beryllium F 18.0904 10 Ne 20.1797 12.0107 | 140057415994 Li Be 9012112 magnesium 18 6941 sodium 11 AI Р 30.97375 26.981536 Na Mg 22.99977 243050 potassium CI Ar 35.453 39.984 krypton 36 Kr 73.904 103.799 Ga edicium 20 Ca Ge As Se 7264 K 39.098340.078 LJ mo their proper position on...