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Chemistry Chapter 5 Flashcards
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Chemistry Chapter 5 Flashcards

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Questions and Answers

The idea of arranging the elements in the periodic table according to their chemical and physical properties is attributed to?

Mendeleev

Mendeleev noticed that properties of elements usually repeated at regular intervals when the elements were arranged in order of increasing?

atomic mass

Mendeleev did not always list elements in his periodic table in order of increasing atomic mass because he grouped together elements with similar?

properties

Mendeleev predicted that the spaces in his periodic table represented?

<p>undiscovered elements</p> Signup and view all the answers

The person whose work led to a periodic table based on increasing atomic number was?

<p>Moseley</p> Signup and view all the answers

The periodic table permits the properties of an element to be predicted before the element is discovered?

<p>true</p> Signup and view all the answers

What are the radioactive elements with atomic numbers from 90 to 103 called?

<p>the actinides</p> Signup and view all the answers

Argon, krypton, and xenon are?

<p>noble gases</p> Signup and view all the answers

The periodic law allows some properties of an element to be predicted based on its?

<p>position in the periodic table</p> Signup and view all the answers

Elements in a group or column in the periodic table can be expected to have similar?

<p>properties</p> Signup and view all the answers

How much greater is the atomic number of the fourth element in groups 1, 2, and 18 than the preceding element?

<p>18</p> Signup and view all the answers

In the pattern 8, 8, 18, __, 32, what number completes the pattern for elements in groups 1, 2, and 18?

<p>18</p> Signup and view all the answers

A horizontal row of blocks in the periodic table is called a?

<p>period</p> Signup and view all the answers

Identify the sublevels in a period that contains 32 elements?

<p>s, p, d, f</p> Signup and view all the answers

How many elements are in a period in which only the s and p sublevels are filled?

<p>8</p> Signup and view all the answers

In what period is cesium, with atomic number 55?

<p>Period 6</p> Signup and view all the answers

In period 3 there are 8 elements. What sublevel(s) is (are) being filled?

<p>s and p</p> Signup and view all the answers

Period 4 contains 18 elements. How many of these elements have electrons in the d sublevel?

<p>16</p> Signup and view all the answers

In what period is calcium, atomic number 20?

<p>Period 4</p> Signup and view all the answers

The s sublevel of the highest occupied energy level varies in the number of electrons it contains?

<p>true</p> Signup and view all the answers

Neutral atoms with an s^2p^6 electron configuration in the highest energy level belong to which block of the periodic table?

<p>p block</p> Signup and view all the answers

The group of 14 f block elements in the sixth period is called?

<p>lanthanides</p> Signup and view all the answers

Within the p-block elements, the elements at the top of the table, compared with those at the bottom, are?

<p>less metallic</p> Signup and view all the answers

The electron configurations of the noble gases from neon to radon in the periodic table make these elements part of the?

<p>p block</p> Signup and view all the answers

Hydrogen is placed separately from other elements in the periodic table because it?

<p>has many unique properties</p> Signup and view all the answers

For groups 13 through 18, the total number of electrons in the highest occupied level equals the group number minus?

<p>10</p> Signup and view all the answers

The electron configuration of an element is [Kr] 4d^6 5s^1. To what group does this element belong?

<p>group 7</p> Signup and view all the answers

Which block in the periodic table contains the alkali metals?

<p>s</p> Signup and view all the answers

The most reactive group of nonmetals is the?

<p>halogens</p> Signup and view all the answers

The group of soft, silvery, reactive metals, all of which have one electron in an s orbital, is known as the?

<p>alkali metals</p> Signup and view all the answers

The first member of the noble gas family, whose highest energy level consists of an octet of electrons, is?

<p>neon</p> Signup and view all the answers

The most characteristic property of the noble gases is that they?

<p>are largely unreactive</p> Signup and view all the answers

One-half the distance between the nuclei of identical atoms bonded together is called the?

<p>atomic radius</p> Signup and view all the answers

What is removed when the ionization energy is supplied to an atom of an element?

<p>an electron</p> Signup and view all the answers

The element that has the greatest electronegativity is?

<p>fluorine</p> Signup and view all the answers

A positive ion is known as a(n)?

<p>cation</p> Signup and view all the answers

In a row in the periodic table, as the atomic number increases, the atomic radius generally?

<p>decreases</p> Signup and view all the answers

Within a group of elements, as the atomic number increases, the atomic radius?

<p>increases</p> Signup and view all the answers

Across a period in the periodic table, atomic radii?

<p>gradually decrease</p> Signup and view all the answers

Which is the best reason that the atomic radius generally increases with atomic number in each group of elements?

<p>the number of occupied energy levels increases</p> Signup and view all the answers

The ionization energies required to remove successive electrons from a mole of calcium atoms are 590 kJ/mol, 1145 kJ/mol, and 6474 kJ/mol. The most common ion of calcium is probably?

<p>Ca^2+</p> Signup and view all the answers

As you move left to right in Period 4 from gallium through bromine, atomic radii?

<p>generally decrease</p> Signup and view all the answers

The force of attraction by Group 1 metals for their valence electrons is?

<p>weak</p> Signup and view all the answers

The electrons available to be lost, gained, or shared when atoms form compounds are called?

<p>valence electrons</p> Signup and view all the answers

The number of valence electrons in Group 1 elements is?

<p>1</p> Signup and view all the answers

In Group 2 elements, the valence electrons are in sublevel?

<p>s</p> Signup and view all the answers

The number of valence electrons in Group 17 elements is?

<p>7</p> Signup and view all the answers

In groups 13 through 18, valence electrons may be in sublevels?

<p>s and p</p> Signup and view all the answers

Across a period, ionization energies of d-block elements generally?

<p>increase</p> Signup and view all the answers

The first electrons to be removed when d-block elements form ions are the?

<p>s electrons</p> Signup and view all the answers

State the Periodic Law.

<p>The physical and chemical properties of an element are the periodic functions of their atomic numbers.</p> Signup and view all the answers

Study Notes

Periodic Table Development

  • Mendeleev is recognized for arranging elements in the periodic table based on chemical and physical properties.
  • He observed that element properties repeat at regular intervals when ordered by atomic mass.
  • Mendeleev prioritized grouping elements by similar properties rather than strictly by atomic mass.
  • He predicted that gaps in his table indicated undiscovered elements.

Modern Periodic Table

  • Moseley's work led to the periodic table organization based on increasing atomic number instead of atomic mass.
  • The periodic law predicts element properties based on their location within the periodic table.
  • Elements in the same group or column exhibit similar chemical properties.

Element Groups and Blocks

  • Radioactive elements with atomic numbers 90 to 103 are termed actinides.
  • Noble gases include argon, krypton, and xenon, noted for their lack of reactivity.
  • The p block comprises noble gases, such as neon to radon, and elements with a s^2p^6 configuration.

Electron Configuration

  • Unfilled sublevels determine the number of elements in a period; periods with 32 elements include s, p, d, and f sublevels.
  • Elements in periods where only the s and p sublevels are filled contain 8 elements.
  • The electron configuration of an element (example: cesium, atomic number 55, is [Xe] 6s^1) indicates its period.

Atomic and Ionic Properties

  • Atomic radius is defined as half the distance between the nuclei of bonded atoms.
  • As atomic number increases in a period, atomic radius generally decreases.
  • In a group, atomic radius increases with increasing atomic number due to additional occupied energy levels.

Ionization Energy and Electronegativity

  • Ionization energy is the energy required to remove an electron from an atom.
  • Calcium's common ion, due to its ionization energies, is likely Ca^2+.
  • Fluorine exhibits the highest electronegativity, making it very reactive in forming compounds.

Valence Electrons

  • Valence electrons are electrons that can be gained, lost, or shared when forming chemical bonds.
  • Group 1 elements have 1 valence electron, while Group 17 elements have 7.
  • In groups 13 to 18, valence electrons reside in s and p sublevels.
  • Across a period, atomic radii decrease while ionization energies typically increase.
  • D-block elements see their first electrons removed from the s sublevel when forming ions.
  • The force of attraction for valence electrons diminishes in Group 1 metals, leading to high reactivity.

Summary of Periodic Law

  • The Periodic Law asserts that physical and chemical properties of elements are periodic functions of their atomic numbers.

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Test your knowledge of Chapter 5 in chemistry with these flashcards. This set focuses on the periodic table and the contributions of Mendeleev to the field. Challenge yourself to remember important definitions and concepts associated with the arrangement of elements.

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