Atomic Properties Quiz
24 Questions
2 Views

Atomic Properties Quiz

Created by
@SincereJasper3476

Podcast

Play an AI-generated podcast conversation about this lesson

Questions and Answers

What happens to atomic radius across a period and down a group?

Atomic radius decreases across a period from left to right and increases down a group from top to bottom.

How does ionization energy change across periods and down groups?

Ionization energy increases across a period from left to right and decreases down a group from top to bottom.

Define electronegativity and its trend in the periodic table.

Electronegativity is the ability of an atom to attract electrons. It increases across a period from left to right and decreases down a group.

What is electron affinity and how does it change across terms in the periodic table?

<p>Electron affinity is the energy change that occurs when an electron is added to a gaseous atom. It generally increases down the groups and decreases across a period from left to right.</p> Signup and view all the answers

Explain the relationship between cations and ionic radius.

<p>Cations, formed by the loss of electrons, are smaller than their neutral atoms due to reduced electron-electron repulsion.</p> Signup and view all the answers

Describe the trend in melting and boiling points from group I to IV.

<p>The melting and boiling points increase from group I to group IV across periods.</p> Signup and view all the answers

What is electropositivity and how does it vary in the periodic table?

<p>Electropositivity is the ability of an atom to lose electrons and form positive ions. It decreases across a period from left to right and increases down a group.</p> Signup and view all the answers

What is the valence electron configuration for alkali metals?

<p>The valence electron configuration for alkali metals is $ns^1$, where $n$ represents the period number.</p> Signup and view all the answers

How does the ionic radius of non-metals change across periods?

<p>The ionic radius of non-metals generally decreases across periods.</p> Signup and view all the answers

Explain the trend in ease of formation of ions for non-metals across periods.

<p>The ease of formation of ions for non-metals increases from Group IV to Group VII across periods due to increasing electron affinity.</p> Signup and view all the answers

What similarities exist between lithium and magnesium regarding their chemical properties?

<p>Lithium and magnesium both form normal oxides and have similar solubility characteristics in water.</p> Signup and view all the answers

How does the metallic character change down the groups of the periodic table?

<p>Metallic character increases as you move down the groups in the periodic table due to decreasing ionization energy.</p> Signup and view all the answers

What is the electron gain trend for halogens as you move down the group?

<p>The ease of gaining electrons decreases for halogens as you move down the group.</p> Signup and view all the answers

Describe the trend in chemical reactivity for alkaline earth metals down the group.

<p>Chemical reactivity of alkaline earth metals increases down the group due to lower ionization energies.</p> Signup and view all the answers

What characteristic do Beryllium and Aluminium share that illustrates diagonal relationships?

<p>Beryllium and Aluminium both exhibit similar behavior in forming compounds with similar stoichiometries.</p> Signup and view all the answers

How does the ionization energy trend across periods affect non-metals?

<p>Ionization energy increases across periods, making it more difficult for non-metals to lose electrons.</p> Signup and view all the answers

What is the trend of ionic radius across the periodic table?

<p>Ionic radius generally decreases across a period due to increasing nuclear charge, which pulls electrons closer to the nucleus.</p> Signup and view all the answers

How does the melting point change from Group I to Group III?

<p>Melting points generally increase from Group I to Group III due to stronger metallic bonds and a transition to giant covalent structures.</p> Signup and view all the answers

Describe the trend in chemical reactivity for non-metals across periods.

<p>Chemical reactivity for non-metals increases from Group IV to Group VII across the periods.</p> Signup and view all the answers

What happens to electron affinity across the periodic table?

<p>Electron affinity increases across periods as elements become more electronegative and better at attracting electrons.</p> Signup and view all the answers

How does atomic size change as you go down a group in the periodic table?

<p>Atomic size increases down a group due to the addition of electron shells, which outweighs the increase in nuclear charge.</p> Signup and view all the answers

Explain the trend of ionization energy across the periodic table.

<p>Ionization energy generally increases across a period as the atomic radius decreases and nuclear charge increases.</p> Signup and view all the answers

What is the relationship between electronegativity and reactivity of non-metals?

<p>Higher electronegativity in non-metals indicates greater ability to attract electrons, making them more reactive.</p> Signup and view all the answers

Describe the changes in thermal stability of compounds from Groups I to VII.

<p>Thermal stability of compounds generally decreases from Group I to III for metals and increases from Group IV to VII for non-metals.</p> Signup and view all the answers

Study Notes

Atomic Properties

  • Electronegativity is an atom's ability to attract electrons and become negatively charged.
  • Electropositivity is an atom's ability to lose electrons and become positively charged.
  • Electron Affinity is the energy change when one mole of electrons is added to one mole of gaseous atoms to form negative ions.
  • Atomic Radius decreases across periods from left to right, but increases down groups from top to bottom.
  • Ionization Energy increases across periods from left to right, but decreases down groups from top to bottom.
  • Electronegativity increases across periods from left to right, but decreases down groups from top to bottom.
  • Electropositivity decreases across periods from left to right, but increases down groups from top to bottom.
  • Electron Affinity decreases across periods and generally increases down groups.
  • Ionic radius decreases for metals across periods and increases for non-metals. Ionic radius generally increases down groups and decreases across periods.
  • Cations are smaller than the neutral atom they are formed from, while anions are larger than the neutral atom.
  • The larger the charge on a cation, the smaller the ionic radius. The larger the charge on an anion, the larger the ionic radius.
  • Ionization Energy increases across periods and decreases down groups.
  • Atomic Radius decreases across periods and increases down groups.

Variation in Physical Properties

  • Melting Point and Boiling Point increase across periods for Group I-III elements, with Group IV elements having the highest values. The trend then decreases for Group V-VII elements. Melting and boiling points decrease down groups for Group I-IV elements, but increase down groups for Group V-VII elements.
  • Ease of Ion Formation decreases across the periods from Group I-III for metals, and increases for non-metals from Group IV-VII. Ease of ion formation increases down the groups for metals and decreases for non-metals.

Diagonal Relationship in Properties

  • Diagonal relationships exist between pairs of diagonally adjacent elements in the second and third periods (e.g., Li and Mg, Be and Al, B and Si).
  • The chemistry of a second-period element often has similarities to the chemistry of the third-period element one column to the right.
  • Charge density is a factor in the diagonal relationship.

Examples of Li-Mg Diagonal Relationship

  • Lithium and Magnesium form normal oxides, while Sodium forms peroxide and superoxides.
  • Lithium is the only Group I element to form a stable nitride (Li3N). Magnesium and other Group II elements also form nitrides.
  • Lithium trioxocarbonate (IV) and Lithium fluoride are sparingly soluble, while corresponding Group II salts are insoluble.
  • Chlorides of Li and Mg are deliquescent and soluble in ethanol. Lithium chloride and magnesium chloride crystallize as hydrated salts.

Variation in Other Physical Properties

  • Melting and Boiling Point trends are influenced by the strength of metallic and covalent bonding, as well as intermolecular forces of attraction.
  • Electrical and Thermal Conductivity decrease across periods but increase down groups. Metals are good conductors, while non-metals are poor conductors.

Variation in Chemical Properties

  • Chemical Properties of elements show periodic variation due to the number of valence electrons.
  • Groups of elements within the same column have similar chemical properties due to similar valence electron configurations.
  • Periods of elements within the same row have different chemical properties.

Chemical Properties Across the Periodic Table

  • Chemical Reactivity: Decreases across periods for metals from Group I-III and increases for non-metals from Group IV-VII. Reactivity increases down groups for metals and decreases down groups for non-metals.
  • Thermal Stability of Compounds: Decreases across periods for metals from Group I-III and increases for non-metals from Group IV-VII. Thermal stability increases down groups for metals and decreases for non-metals.
  • Ease of Ion Formation: Decreases across periods for metals from Group I-III and increases for non-metals from Group IV-VII. Ease of ion formation increases down groups for metals and decreases for non-metals.
  • Metallic Properties: Decrease across periods and increase down groups.
  • Non-Metallic Properties: Increase across periods and decrease down groups.

Groups of Elements with Similar Properties

  • Alkali Metals (Group 1)
  • Alkaline Earth Metals (Group 2)
  • Halogens ( Group 7)
  • Noble Gases (Group 0)

Studying That Suits You

Use AI to generate personalized quizzes and flashcards to suit your learning preferences.

Quiz Team

Related Documents

Chemistry Past Paper - SS 2 - First Term

Description

Test your knowledge of atomic properties such as electronegativity, electropositivity, electron affinity, atomic radius, and ionization energy. This quiz covers key concepts and trends within the periodic table. Perfect for students studying chemistry!

More Like This

Use Quizgecko on...
Browser
Open
Browser
Browser