Electron Affinity Lowersixth Science Chemistry

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Electron Affinity Lowersixth Science Chemistry


Froggy Jumps Electron Affinity Lowersixth Science ChemistryVersión en línea Test your understanding of periodic trends in chemistry. por YAKILI LMS 1 What does ionization energy measure? a Energy released when an atom forms a bond b Energy required to remove the outermost electron c Energy gained when electrons are added 2 How does ionization energy generally change across a period? a Increases from left to right b Stays the same c Decreases from left to right 3 How does ionization energy generally change down a group? a Stays the same b Decreases as you go down c Increases as you go down 4 Electron affinity is best described as the energy change when an atom ______? a Releases energy on bonding b Gains an electron c Loses an electron 5 Electron affinity is the converse of which concept? a Electronegativity b Atomic radius c Ionization energy 6 What is the general trend of electron affinity across a period? a Becomes more positive b Stays the same c Becomes more negative 7 Which element typically has a very high (negative) electron affinity? a Noble gas such as neon b Chlorine c Helium 8 Which factor primarily drives periodic trends in ionization energy? a Effective nuclear charge b Atomic mass c Ion charge 9 What happens to ionization energy when an electron is removed from a positively charged ion? a It requires less energy for the next removal b It requires more energy for the next removal c It becomes zero 10 Which group tends to have highest first ionization energy in the period? a Alkali metals b Alkaline earth metals c Noble gases 11 The term 'periodic trend' refers to predictable changes across the periodic table in: a Ionization energy and electron affinity b Atomic radius only c Atomic mass only 12 Which element has the smallest atomic radius within a period? a Sodium b Potassium c Fluorine 13 As you move down a group, ionic radius generally: a Stays the same b Increases c Decreases 14 Which statement is true about electron affinity in noble gases? a All noble gases have identical electron affinity b Noble gases have very low or positive electron affinity c All noble gases have highly negative electron affinity 15 Which factor reduces ionization energy across a period? a Decreased protons b Increased nuclear charge with constant shielding c Increased shielding 16 Which member of the second period has the highest first ionization energy? a Beryllium b Lithium c Neon 17 Electron affinity becomes less negative for which type of element? a Metalloids b Noble gases c Nonmetals 18 Which statement describes a general trend for electron affinity across a period? a Becomes more positive b Stays constant c Becomes more negative from left to right for many elements 19 What makes alkali metals have low ionization energies? a Only one valence electron loosely held b Very strong nuclear charge c Many unpaired electrons 20 Which element has a notably high first ionization energy due to lack of electron shielding? a Krypton b Sodium c Helium 21 Which of the following best describes electron affinity for chlorine? a It releases energy when gaining an electron b It consumes energy to lose an electron c It is undefined 22 Which trend is true for ionization energy when moving from left to right across a period? a Ionization energy decreases b Ionization energy generally increases c Stays same 23 If an atom has a high ionization energy, it tends to form ions by: a Losing electrons easily b Gaining electrons c Not forming ions 24 What is a consequence of high effective nuclear charge on an atom? a Lower protons count b Tighter hold on valence electrons c Looser hold on valence electrons 25 Which group has the most negative electron affinity in period 2? a Noble gases b Chlorine family analogs trend c Alkali metals 26 Which factor contributes to decreasing ionization energy down a group? a Decreasing shielding b Increasing atomic size c Increasing nuclear charge 27 Between sodium and chlorine, which has higher first ionization energy? a Chlorine b Sodium c Both same 28 Which statement best describes ionization energy of alkaline earth metals compared to alkali metals? a Alkaline earth metals have higher ionization energy b Same as alkali metals c Lower than alkali metals 29 What happens to electron affinity when an atom fills its valence shell? a Becomes more negative b Remains highly negative c Electron affinity becomes less negative 30 Which trend is observed for atomic radius across a period? a Radius stays same b Radius decreases c Radius increases 31 Which element would have the highest first ionization energy among period 2 elements? a Neon b Lithium c Beryllium 32 What is the relationship between ionization energy and electron affinity for a strong nonmetal? a High ionization energy and high electron affinity b Low both c High ionization energy but low electron affinity 33 Why do halogens have high electron affinities? a They already have stable shells b They are noble gases c They need one more electron to complete a shell 34 Which statement about electron affinity is always true? a It measures energy to remove a proton b It is the energy released when an atom forms a bond c It is the energy change when adding an electron 35 Which trend is observed for ionization energy within group 17 (halogens) down the column? a Ionization energy decreases b Ionization energy increases c Stays constant 36 Which factor most influences electron affinity in a periodic table element? a Valence electron configuration b Melting point c Atomic weight 37 Which element has a relatively low electron affinity? a Chlorine b Fluorine c Noble gas such as neon 38 Which is true about ionization energy and shielding? a Shielding raises ionization energy b Shielding has no effect c Increased shielding lowers ionization energy 39 Which statement best defines a periodic trend? a Only within a period b Consistent change across periods and groups c Random changes 40 Which element in period 3 has the highest first ionization energy? a Magnesium b Sodium c Neon does not belong to period 3; Ar is period 3 41 Electron affinity is most positive for which type of element? a Halogens b Alkali metals c Noble gases 42 Which statement is false about periodic trends? a Ionization energy increases down a group b Radius decreases across a period c Ionization energy decreases across a period 43 What happens to ionization energy when an outer electron is removed? a Energy required decreases for subsequent removals b Removals become impossible c Energy required for subsequent removals increases 44 Which factor causes the drop in ionization energy down a group? a Increasing protons with same shielding b Decreasing radius c Increasing atomic size and shielding 45 Which element has the most negative electron affinity in period 2? a Beryllium b Fluorine c Lithium 46 In a short answer: define electron affinity in one line. a Energy change when an atom gains an electron b Energy required to remove a proton c Energy change when an atom loses an electron 47 Which trend is observed for atomic radius across a period? a Radius increases b Radius decreases c Stays the same 48 Which element commonly has a high ionization energy due to closed shells? a Sodium b Neon c Potassium 49 Which statement links ionization energy and electron affinity? a Both relate to electron interactions with the nucleus b They are unrelated properties c Only ionization energy depends on shielding 50 Which group typically has the least tendency to gain electrons? a Noble gases b Alkali metals c Halogens

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Electron Affinity Lowersixth Science ChemistryVersión en línea

por YAKILI LMS

What does ionization energy measure?

How does ionization energy generally change across a period?

How does ionization energy generally change down a group?

Electron affinity is best described as the energy change when an atom ______?

Electron affinity is the converse of which concept?

What is the general trend of electron affinity across a period?

Which element typically has a very high (negative) electron affinity?

Which factor primarily drives periodic trends in ionization energy?

What happens to ionization energy when an electron is removed from a positively charged ion?

Which group tends to have highest first ionization energy in the period?

The term 'periodic trend' refers to predictable changes across the periodic table in:

Which element has the smallest atomic radius within a period?

As you move down a group, ionic radius generally:

Which statement is true about electron affinity in noble gases?

Which factor reduces ionization energy across a period?

Which member of the second period has the highest first ionization energy?

Electron affinity becomes less negative for which type of element?

Which statement describes a general trend for electron affinity across a period?

What makes alkali metals have low ionization energies?

Which element has a notably high first ionization energy due to lack of electron shielding?

Which of the following best describes electron affinity for chlorine?

Which trend is true for ionization energy when moving from left to right across a period?

If an atom has a high ionization energy, it tends to form ions by:

What is a consequence of high effective nuclear charge on an atom?

Which group has the most negative electron affinity in period 2?

Which factor contributes to decreasing ionization energy down a group?

Between sodium and chlorine, which has higher first ionization energy?

Which statement best describes ionization energy of alkaline earth metals compared to alkali metals?

What happens to electron affinity when an atom fills its valence shell?

Which trend is observed for atomic radius across a period?

Which element would have the highest first ionization energy among period 2 elements?

What is the relationship between ionization energy and electron affinity for a strong nonmetal?

Why do halogens have high electron affinities?

Which statement about electron affinity is always true?

Which trend is observed for ionization energy within group 17 (halogens) down the column?

Which factor most influences electron affinity in a periodic table element?

Which element has a relatively low electron affinity?

Which is true about ionization energy and shielding?

Which statement best defines a periodic trend?

Which element in period 3 has the highest first ionization energy?

Electron affinity is most positive for which type of element?

Which statement is false about periodic trends?

What happens to ionization energy when an outer electron is removed?

Which factor causes the drop in ionization energy down a group?

Which element has the most negative electron affinity in period 2?

In a short answer: define electron affinity in one line.

Which trend is observed for atomic radius across a period?

Which element commonly has a high ionization energy due to closed shells?

Which statement links ionization energy and electron affinity?

Which group typically has the least tendency to gain electrons?