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...
1. Describe and explain the trend of the ionization energy of elements: (i) across a period;...
1. Describe and explain the trend of the ionization energy of elements: (i) across a period; (ii) down a group, in the periodic table. 2. Reactivity of alkali metals (Group 1A) increases from top to bottom down the group, but the reactivity of halogen (Group 7A) decreases from top to bottom down the group. Explain why the difference.
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 increase as you move left to right across the periodic...
Explain why the effective nuclear charge increase as you move left to right across the periodic table and how electronegativity depends on the effective nuclear charge. Thank you!
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 ?
What is the trend for …. When you go across the period? Down a family? For...
What is the trend for …. When you go across the period? Down a family? For each trend, explain in your own words what it means and/or why it is. a) atomic size? b) ionization energy? c) electron affinity? Which should be larger according to the general trend? Explain. Li, Na? K or K+? Cl or Cl-? P or S?
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
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 (Groups I-VIII) for a) sizes of atoms, cations, anions (same charge) b) ionization energies c) electron affinities d) electronegativities
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