Differentiates between ionisation potential and electron affinity?

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Rumana Israr

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The minimum energy required to remove the loosely packed electron from an isolated gaseous atom is known as ionisation energy. Whereas ,electron affinity is the amount of energy released when an atom is added into an isolated gaseous atom.
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๐Ÿ”น Ionisation Potential (Ionisation Energy) • Definition: Energy required to remove an electron from a neutral gaseous atom. • Process: X(g) \rightarrow X^+(g) + e^- • Nature: Always positive (energy is absorbed). • What it measures: How tightly an atom holds its electrons. ...
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๐Ÿ”น Ionisation Potential (Ionisation Energy) • Definition: Energy required to remove an electron from a neutral gaseous atom. • Process: X(g) \rightarrow X^+(g) + e^- • Nature: Always positive (energy is absorbed). • What it measures: How tightly an atom holds its electrons. • Trend: • Increases across a period (→) • Decreases down a group (↓) • Example: Removing an electron from sodium requires energy. โธป ๐Ÿ”น Electron Affinity • Definition: Energy released when an electron is added to a neutral gaseous atom. • Process: X(g) + e^- \rightarrow X^-(g) • Nature: Usually negative (energy is released). • What it measures: Tendency of an atom to gain an electron. • Trend: • Increases across a period (→) • Decreases down a group (↓) • Example: Chlorine releases energy when gaining an electron. read less
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Ionization potential (IE) is the energy required to remove an electron from a gaseous atom (endothermic), forming a positive ion. Electron affinity (EA) is the energy released when an electron is added to a gaseous atom (typically exothermic), forming a negative ion. IE measures tendency to lose...
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Ionization potential (IE) is the energy required to remove an electron from a gaseous atom (endothermic), forming a positive ion. Electron affinity (EA) is the energy released when an electron is added to a gaseous atom (typically exothermic), forming a negative ion. IE measures tendency to lose electrons; EA measures tendency to gain electrons. read less
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Ionisation Potential (Ionisation Energy) Definition: Energy required to remove an electron from an isolated gaseous atom Key Points: Always endothermic (energy is absorbed) Measures how tightly an atom holds its electrons Higher value → harder to remove electron Increases across a period,...
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Ionisation Potential (Ionisation Energy) Definition: Energy required to remove an electron from an isolated gaseous atom Key Points: Always endothermic (energy is absorbed) Measures how tightly an atom holds its electrons Higher value → harder to remove electron Increases across a period, decreases down a group Electron Affinity Definition: Energy released when an electron is added to an isolated gaseous atom. Key Points: Usually exothermic (energy is released) Measures tendency to gain an electron Higher (more negative) value → greater tendency to accept electron Generally increases across a period (with some exceptions) read less
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Ionization potential (IP) is the energy required to remove an electron from a gaseous atom, creating a positive ion, while electron affinity (EA) is the energy released (or absorbed) when adding an electron to a gaseous atom to create a negative ion. IP is always endothermic (positive), while EA is generally...
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Ionization potential (IP) is the energy required to remove an electron from a gaseous atom, creating a positive ion, while electron affinity (EA) is the energy released (or absorbed) when adding an electron to a gaseous atom to create a negative ion. IP is always endothermic (positive), while EA is generally exothermic (negative). Here is the breakdown of differences: Definition: Ionization Potential (IP): Amount of energy required to remove an electron from the outermost shell of an isolated gaseous atom, forming a cation ( A+IP→A++e− ๐ด+IP→๐ด++๐‘’− ). Electron Affinity (EA): Amount of energy released (typically) when a neutral gaseous isolated atom accepts an electron to form an anion ( A+e−→A−+EA ๐ด+๐‘’−→๐ด−+EA ). Energy Flow: IP: Energy is absorbed by the system (Endothermic). EA: Energy is released by the system (Exothermic). Periodic Trends: IP: Increases across a period (left to right) and decreases down a group. EA: Becomes more negative (greater magnitude) across a period and less negative (smaller magnitude) down a group. Key Indicator: IP indicates the tendency to lose electrons (metallic character). EA indicates the tendency to gain electrons (non-metallic character). read less
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Law student trained with 1year of experience in taking Business studies and English

Ionization potential (IE) is the energy required to remove an electron from a gaseous atom (endothermic), forming a positive ion. In contrast, electron affinity (EA) is the energy released when an electron is added to a gaseous atom (typically exothermic), forming a negative ion. IE measures tendency...
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Ionization potential (IE) is the energy required to remove an electron from a gaseous atom (endothermic), forming a positive ion. In contrast, electron affinity (EA) is the energy released when an electron is added to a gaseous atom (typically exothermic), forming a negative ion. IE measures tendency to lose electrons; EA measures tendency to gain electrons. read less
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Ionisation potential is the energy needed to remove an electron from an atom, while electron affinity is the energy released when an electron is added to an atom. Think of it like a tug-of-war: ionisation potential is like pulling an electron away, and electron affinity is like the atom welcoming an...
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Ionisation potential is the energy needed to remove an electron from an atom, while electron affinity is the energy released when an electron is added to an atom. Think of it like a tug-of-war: ionisation potential is like pulling an electron away, and electron affinity is like the atom welcoming an electron with open arms ๐Ÿ™. Want more details? read less
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Electron affinity can reflect to the ability of an atom to gain electrons, the smaller the first electron affinity the easier an atom gains electrons, the greater the electron affinity the weaker is the ability of an atom to gain electrons. The ionization energy shows the ability of an atom to lose its...
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Electron affinity can reflect to the ability of an atom to gain electrons, the smaller the first electron affinity the easier an atom gains electrons, the greater the electron affinity the weaker is the ability of an atom to gain electrons. The ionization energy shows the ability of an atom to lose its electrons read less
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Physics tutor for 9th to 12th (CBSE, ICSE, NEET , JEE)

Ionisation Energy:- Energy required to remove an electron from an isolated gaseous atom atom---> cation + e- Electron Affinity :- Energy change when an electron is added to a neutral gaseous atom. atom+ e- ----> Anion
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Ionisation Energy:- Energyrequired to remove an electron from an isolated gaseous atom atom---> cation + e- Electron Affinity :-Energy change when an electron is added to a neutral gaseous atom. atom+ e- ----> Anion read less
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Ionization Potential (IP) and Electron Affinity (EA) are both measures of an atom's energy changes regarding electrons, but they describe opposite processes. In short: IP is the energy required to remove an electron (forming a positive ion), while EA is the energy released when adding an electron (forming...
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Ionization Potential (IP) and Electron Affinity (EA) are both measures of an atom's energy changes regarding electrons, but they describe opposite processes. In short: IP is the energy required to remove an electron (forming a positive ion), while EA is the energy released when adding an electron (forming a negative ion). read less
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