Domanda del libro di testo
Choose the larger atom in each pair. a. I or In b. Sb or P c. Te or Br d. S or Ge
Ch.9 - Periodic Properties of the Elements
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
Non è quello che usi tu?Cambia libro di testoScegli un libro di testo diverso
TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Capitolo 9, Problema 63
Choose the larger atom in each pair. a. P or O b. Si or Sn c. S or Sb d. B or N
Guida verificata passo dopo passo1
Step 1: Understand the concept of atomic size. Atomic size generally increases as you move down a group in the periodic table and decreases as you move across a period from left to right.
Step 2: Compare the atomic sizes for each pair by locating them on the periodic table. For pair (a) P or O, both are in the same period, so compare their positions across the period.
Step 3: For pair (b) Si or Sn, note that they are in the same group. Atomic size increases as you move down a group, so compare their positions vertically.
Step 4: For pair (c) S or Sb, they are in different periods and groups. Consider both the group and period trends to determine which is larger.
Step 5: For pair (d) B or N, both are in the same period. Compare their positions across the period to determine which is larger.
Risposta video verificata per un problema simile:
Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
2mConcetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
Atomic Size
Atomic size refers to the distance from the nucleus to the outermost electron shell of an atom. Generally, atomic size increases down a group in the periodic table due to the addition of electron shells, while it decreases across a period from left to right due to increased nuclear charge, which pulls electrons closer to the nucleus.
Video consigliato:
Percorso guidato
02:10
Atom Structure
Periodic Trends
Periodic trends are patterns observed in the periodic table that describe how certain properties of elements change across periods and down groups. Key trends include atomic radius, ionization energy, and electronegativity, which help predict the behavior of elements in chemical reactions and their relative sizes.
Video consigliato:
Percorso guidato
00:38Periodic Trends
Comparison of Elements
When comparing elements, it is essential to consider their positions in the periodic table. Elements in the same group typically have similar properties, while those in the same period show trends in size and reactivity. Understanding these relationships allows for accurate comparisons of atomic sizes among different elements.
Video consigliato:
Percorso guidato
02:35Elemental Forms of Elements
Pratica correlata
Domanda del libro di testo
In Section 3.6, we estimated the effective nuclear charge on beryllium's valence electrons to be slightly greater than 2+. What would a similar treatment predict for the effective nuclear charge on boron's valence electrons? Would you expect the effective nuclear charge to be different for boron's 2s electrons compared to its 2p electron? In what way? (Hint: Consider the shape of the 2p orbital compared to that of the 2s orbital.)
1059
views
1
rank
Domanda del libro di testo
If core electrons completely shielded valence electrons from nuclear charge (i.e., if each core electron reduced nuclear charge by 1 unit) and if valence electrons did not shield one another from nuclear charge at all, what would be the effective nuclear charge experienced by the valence electrons of each atom? b. Ca
528
views
Domanda del libro di testo
If core electrons completely shielded valence electrons from nuclear charge (i.e., if each core electron reduced nuclear charge by 1 unit) and if valence electrons did not shield one another from nuclear charge at all, what would be the effective nuclear charge experienced by the valence electrons of each atom? c. O d. C
2895
views
1
rank