Periodic trends
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Atomic radius decreases and ionization energy increases when moving from left to right across a period. The nuclear charge increases while shielding remains constant, strengthening the attraction between electrons and the nucleus. Atomic radius increases and ionization energy decreases when moving down a group, as the valence electrons are farther from the nucleus due to additional electron shells providing shielding.
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2. Specifically, it notes that atomic size decreases across periods as nuclear charge increases, while increasing down groups as additional shells are added. Ionization energy and electronegativity both increase from left to right as nuclear charge increases, while decreasing down groups as electrons are farther from the nucleus. Metallic character increases down groups and decreases across periods.
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The document discusses several periodic trends, including how atomic radius, ionic radius, ionization energy, and electronegativity change across periods and down groups in the periodic table.
[1] Atomic radius decreases and ionization energy increases when moving across a period as nuclear charge increases, while trends are opposite when moving down a group as additional energy levels are added.
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[3] Electronegativity also decreases down groups as the distance between nucleus and electrons increases, but increases across periods as nuclear charge rises.
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1) Atomic radius decreases across a period as atomic number increases, leading to higher effective nuclear charge and stronger attraction of the nucleus. Atomic radius increases down a group as shielding electrons increase.
2) Ionization energy increases across a period as effective nuclear charge increases, making it harder to remove electrons. Ionization energy decreases down a group as shielding increases and atomic radius gets larger.
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1) Atomic radius generally increases down a group and decreases across a period due to shielding effects of additional electron shells and increasing nuclear charge, respectively.
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1. The document discusses several periodic trends including atomic radius, ionization energy, and electronegativity. It explains that atomic radius decreases left to right within a period and increases down a group. Ionization energy generally increases left to right within a period and decreases down a group. Electronegativity increases left to right within a period and decreases down a group.
2. The document also discusses ionic radius trends, explaining that the size of positive ions decreases left to right within a period while the size of negative ions increases. Ionic radius increases down a group for both positive and negative ions.
3. The octet rule is mentioned as determining what types of ions atoms will form in order to acquire
Periodicity
The document discusses periodicity and how properties vary across periods and down groups in the periodic table. It specifically focuses on Period 3 elements (Na to Ar). Key points:
1) Atomic radius decreases across Period 3 as nuclear charge increases, attracting electrons more strongly. Radius increases down groups as atomic size increases.
2) Ionization energy generally increases across Period 3 as nuclear charge increases, requiring more energy to remove electrons. It decreases down groups as distance from nucleus increases.
3) Melting/boiling points are highest for metals/covalent networks and lower for weak molecular bonds. Electrical conductivity is highest for metals and lowest for nonmetals.
Periodic Trends
The document discusses periodic trends in chemical and physical properties revealed by the periodic table. It examines six key trends: atomic number, atomic mass, atomic radius, electronegativity, ionization energy, and reactivity. For each trend, it describes how the property changes as you move down groups or across periods on the periodic table, enabling predictions about an element's chemical behavior.
Chemistry 210 Descriptive Chemistry.pptx
This document discusses trends in properties of elements across the periodic table, including:
1. Atomic and ionic radii generally increase down a group and decrease across a period, with exceptions due to electronic configuration effects like the lanthanide contraction.
2. Ionization energies decrease down a group and increase across a period as it becomes easier to remove electrons from larger atoms with more diffuse orbitals.
3. Electronegativity increases across a period as nuclear charge increases, and decreases down a group as atomic size increases.
Periodic Relationships
There are observable trends in the physical and chemical properties of elements across periods and down groups in the periodic table. As you move across a period, atomic radius decreases due to the increasing effective nuclear charge pulling the valence electrons closer. Down groups, atomic radius increases as each successive energy level is farther from the nucleus. Ionization energy generally increases across periods as effective nuclear charge increases, and decreases down groups as the valence electrons are farther from the nucleus. Electron affinity increases across periods but decreases down groups. Oxidation states can be used to keep track of electrons in compounds and ions.
Properties of periodic table by Saliha Rais
The presentation "Properties of Periodic Table" is prepared for grade IX students. The slide show includes a brief description on the properties of elements in the periodic table, that shifts periodically, hence explaining the concept of periodicity. the main topics include Atomic Radii, Ionization energy, Electron affinity and Electronegativity.
Periodic Trends
1) Periodic trends refer to how properties of elements change regularly when arranged in order of increasing atomic number. These properties include atomic radius, ionization energy, and electronegativity.
2) Atomic radius generally increases moving left to right and decreases moving up a group. Ionization energy follows the opposite trend, increasing up and right as atomic radius decreases. Electronegativity also increases up and right.
3) The trends are due to changes in the number of protons, electrons, and shielding of core electrons that affect the attraction between electrons and the nucleus across the periodic table.
Periodic Trends
1) Periodic trends refer to how properties of elements change regularly when arranged in order of increasing atomic number. These properties include atomic radius, ionization energy, and electronegativity.
2) Atomic radius generally increases moving left to right and decreases moving up a group. Ionization energy follows the opposite trend, increasing up and right as atomic radius decreases. Electronegativity also increases up and right.
3) The trends are due to changes in the number of protons, electrons, and shielding of core electrons that affect the attraction between electrons and the nucleus across the periodic table.
Periodic trends
Here are the answers to your questions:
1. Shielding of nuclear charge remains constant as you move across a period or down a group since the number of electron shells remains the same.
2. Atomic size decreases as you move across a period due to increased nuclear charge, and increases as you move down a group due to additional electron shells providing more shielding.
3. Ions form when atoms gain or lose electrons. Cations form when atoms lose electrons, becoming positively charged. Anions form when atoms gain electrons, becoming negatively charged.
4. Ionization energy is the minimum amount of energy required to remove an electron from a neutral gaseous atom.
5. Ionization energy increases
Periodic Table 5
The document discusses several periodic properties of elements including atomic radius, ionization energy, and electronegativity. It explains that atomic radius decreases across a period as nuclear charge increases but increases down a group as electron shielding increases. Ionization energy generally increases across a period as it becomes harder to remove electrons but decreases down a group as electrons are farther from the nucleus. Electronegativity also increases across a period as nuclear attraction increases.
periodic table and periodicity
Grade 10 CAPS-aligned Periodicity notes. Looks at ionisation energy, electron affinity, electronegativity and atomic radii.
Classification of elements & periodicity in properties
The document discusses periodic trends in properties such as atomic radius, ionization energy, and electronegativity. It explains Mendeleev's periodic table and how modern periodic law arranges elements based on atomic number instead of atomic mass. Periodicity in properties occurs because similar electronic configurations repeat at regular intervals as atomic number increases. Atomic radius generally decreases across a period as nuclear charge increases, and increases down a group as more shells are added. Ionization energy is the energy required to remove an electron from an atom, and is directly proportional to nuclear charge and inversely proportional to size and shielding effects.
Chemistry- JIB Topic 7 Periodicity
The document discusses several key concepts in chemistry including periodic trends in properties, ionization energy, electron affinity, and the behavior of cations, anions, and oxides. Specifically, it explains that ionization energy increases across a period as nuclear charge increases but decreases down a group as electrons experience more shielding. It also describes how cations are smaller than their parent atoms while anions are larger due to electron repulsion. Finally, it summarizes periodic trends in physical and chemical properties within and across periods.
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Periodic trends
- 1. Periodic Trends Jeremy Elwood Cohort Q
- 2. Part I – Atomic Size
- 7. The Periodic Table and Atomic Radius
- 10. Part II – Ionization Energy
- 16. Summary Atomic Radius decreases Ionization energy increases Electronegativity increases Atomic radius increases Ionization energy decreases Electronegativity decreases