Atomic Properties Quiz

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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

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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)

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