1. Explain why the general trend exists for elements getting smaller as you move across a...
1. Explain why the general trend exists for elements getting smaller as you move across a period on the periodic table.
2. Explain the importance of the VSEPR Theory.
Homework Answers
1. when you move across the period in periodic table no of electrons will increase but valency shell wont increase so attraction between the nucleas and electrons will increase this results the decrease the size
2. VESPER theory means Valence Shell Electron Pair Repulsion theory thert theory explains the shape and structure of the molecule
it also explans the no of lone pairs and bond pairs of the electrons at partucular atom
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1. Explain why the general trend exists for elements getting
smaller as you move across a...
can someone help me to answer those questions 8. Explain the trend as you move across...
can someone help me to answer those questions
8. Explain the trend as you move across a row of the periodic table for each of the following some properties using your understanding of effective nuclear charge. Atomic radius b. Ionization energy 6. Electronegativity STOP Model 2 - The Alkali Metals Pare Atomic Number Core Charge Atomic Radius 1st lonization Energy Electro- negativity Lithium 0.91 Sodium 152 pm 186 pm 227 pm 520 kJ/mole 496 kJ/mole 419 kJ/mole 0.87 0.73 Potassium...
- Parta Explain why atomic radius decreases as you move to the right across a period...
- Parta Explain why atomic radius decreases as you move to the right across a period for main-group elements but not for transition elements Match the words in the left column to the appropriate blanks in the sentences on the right Reset Help proton larger As you move to the right across a row in the periodic table for the main-group elements, the effective nudear charge (Zl) experienced by the electrons in the outermost principal energy level resulting in a...
What is the general trend in ionization energy across a row on the periodic table? Using...
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
Explain why the effective nuclear charge increases across a row for the main group elements, but...
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...
34. Explain the general trend for atomic radius going across a period; to the right. 35....
34. Explain the general trend for atomic radius going across a period; to the right. 35. Explain the general trend in atomic radius going down a group.
12. Give the general trend in the periodic table (period, group) for the main group elements...
12. Give the general trend in the periodic table (period, group) for the main group elements (Groups I-VIII) for a) sizes of atoms, cations, anions (same charge) b) ionization energies c) electron affinities d) electronegativities
1) Please use VSEPR theory, explain why the smallest bond angles in IF3 are smaller than...
1) Please use VSEPR theory, explain why the smallest bond angles in IF3 are smaller than the bond angles in NF3 which are in turn smaller than the bond angles in BF3. just few sentence to explain, thank you! 2)In the Y3+ cation, in its ground state, how many electrons have ml = 0 ?
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For the main group elements,in general, upon going from left to right across a period of...
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__
- Class period! Unit 4: Periodic Trends "lonization Energy Trend" - Wksh # 4 2 Directions:...
- 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....
can someone help me to answer those questions
8. Explain the trend as you move across a row of the periodic table for each of the following some properties using your understanding of effective nuclear charge. Atomic radius b. Ionization energy 6. Electronegativity STOP Model 2 - The Alkali Metals Pare Atomic Number Core Charge Atomic Radius 1st lonization Energy Electro- negativity Lithium 0.91 Sodium 152 pm 186 pm 227 pm 520 kJ/mole 496 kJ/mole 419 kJ/mole 0.87 0.73 Potassium...
- Parta Explain why atomic radius decreases as you move to the right across a period for main-group elements but not for transition elements Match the words in the left column to the appropriate blanks in the sentences on the right Reset Help proton larger As you move to the right across a row in the periodic table for the main-group elements, the effective nudear charge (Zl) experienced by the electrons in the outermost principal energy level resulting in a...
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
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12. Give the general trend in the periodic table (period, group) for the main group elements (Groups I-VIII) for a) sizes of atoms, cations, anions (same charge) b) ionization energies c) electron affinities d) electronegativities
- 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....
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