Honors Unit 3: The Electron and Periodic Table
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Questions and Answers

Which of the following properties is not characteristic of metals?

  • Luster (shiny)
  • Good conductors of heat and electricity
  • Brittle and shatter when hit (correct)
  • Malleable and ductile

What type of elements can both gain and lose electrons to form ions?

  • Metals (correct)
  • Metalloids
  • Nonmetals
  • All of the above

Which sample is most likely to be a nonmetal based on its conductivity?

  • Sample B - Light bulb does not light (correct)
  • Sample B - Malleable
  • Sample A - Light bulb lights
  • Sample C - Light bulb lights

In terms of physical properties, which statement is true about metalloids?

<p>Exhibit properties of both metals and nonmetals (D)</p> Signup and view all the answers

What procedure would you use to test for malleability of a sample?

<p>Touch the sample to see if it bends (B)</p> Signup and view all the answers

What is a unique property of nonmetals compared to metals?

<p>They usually exist as gases (C)</p> Signup and view all the answers

Which of the following statements describes metals in terms of electron behavior?

<p>They lose electrons to form cations (B)</p> Signup and view all the answers

Which statement most accurately describes the appearance of metals?

<p>They have high luster and are generally shiny (D)</p> Signup and view all the answers

What is the noble gas that comes before Aluminum (Al)?

<p>Neon (Ne) (B)</p> Signup and view all the answers

What is the correct shorthand electron configuration for Strontium (Sr)?

<p>[Kr] 5s2 (A)</p> Signup and view all the answers

Determine the correct noble gas configuration for tellurium (Te).

<p>[Kr] 5s2 4d10 5p4 (B)</p> Signup and view all the answers

What should the sum of the superscripts equal to for an element with atomic number 20?

<p>20 (B)</p> Signup and view all the answers

Which atom among the following has the greatest shielding effect?

<p>Rb (C)</p> Signup and view all the answers

What is the electron configuration for Zinc (Zn)?

<p>[Ar] 4s2 3d10 (B), [Ar] 4s2 3d10 (C)</p> Signup and view all the answers

What is the effective nuclear charge (Z_eff) for Al?

<p>3 (A)</p> Signup and view all the answers

If the size of an atom increases, which statement is true about its ionization energy?

<p>It decreases. (D)</p> Signup and view all the answers

Which noble gas is used in the configuration of Arsenic (As)?

<p>Argon (Ar) (B)</p> Signup and view all the answers

Which atom will have a stronger hold on its electrons?

<p>Cl (A)</p> Signup and view all the answers

Identify the electron orbital notation for Gallium (Ga).

<p>[Ar] 4s23d104p1 (B)</p> Signup and view all the answers

What is the noble gas configuration for Mercury (Hg)?

<p>[Xe] 6s2 4f14 5d10 (D)</p> Signup and view all the answers

In the alkali metal group, which of the following statements is true regarding atomic radius?

<p>Atomic radius increases down the group. (C)</p> Signup and view all the answers

Which of the following correctly describes electronegativity trends across a period?

<p>Electronegativity increases. (C)</p> Signup and view all the answers

If an atom has greater electron affinity, what can be inferred about its behavior?

<p>It adds electrons easily. (C)</p> Signup and view all the answers

What would be expected if the atomic radius decreases?

<p>Ionization energy increases. (A)</p> Signup and view all the answers

What is the electron configuration for Sodium?

<p>1s22s22p63s1 (B)</p> Signup and view all the answers

Which rule states that no two electrons will have the same spin?

<p>Pauli’s Exclusion Principle (D)</p> Signup and view all the answers

What is the valence shell for Bromine?

<p>4 (A)</p> Signup and view all the answers

Which group of elements in the periodic table is characterized as reactive nonmetals?

<p>Halogens (C)</p> Signup and view all the answers

What is the noble gas configuration for Oxygen?

<p>[He] 2s22p4 (A)</p> Signup and view all the answers

What does the Aufbau Principle state regarding electron configurations?

<p>Electrons should always fill the lowest energy orbitals first. (A)</p> Signup and view all the answers

Which of the following best describes alkali metals?

<p>Reactive, soft metallic solids that are lustrous (A)</p> Signup and view all the answers

Why does strontium have a larger atomic radius compared to magnesium?

<p>More electron shells (C)</p> Signup and view all the answers

How many valence electrons does Calcium (atomic # 20) have?

<p>2 (A)</p> Signup and view all the answers

Which of the following describes the characteristics of nonmetals?

<p>Solids, liquids, and gases that are brittle (B)</p> Signup and view all the answers

Which rule explains that no two electrons in the same orbital can have the same spin?

<p>Pauli Exclusion Principle (C)</p> Signup and view all the answers

What is the correct electron configuration for Arsenic (atomic # 33)?

<p>1s22s22p63s23p64s23d104p3 (C)</p> Signup and view all the answers

What is the significance of having 8 valence electrons in an atom?

<p>It signifies a stable electron configuration. (C)</p> Signup and view all the answers

According to Hund's Rule, what must occur within a set of orbitals?

<p>Each orbital must contain one electron before pairing begins. (A)</p> Signup and view all the answers

How many total electrons does Magnesium (Mg) have based on its configuration 1s22s22p63s2?

<p>12 (D)</p> Signup and view all the answers

In noble gas notation, which noble gas is used as the starting point for Argon (atomic # 18)?

<p>Neon (B)</p> Signup and view all the answers

What is the valence shell for Boron (atomic # 5)?

<p>2 (B)</p> Signup and view all the answers

Why does calcium have a larger atomic radius than bromine?

<p>Bromine's nuclear attraction pulls electrons in closer, making it smaller. (C)</p> Signup and view all the answers

What explains the larger size of the sulfide anion compared to the sulfur atom?

<p>The sulfide anion has gained electrons, leading to increased electron-electron repulsions. (C)</p> Signup and view all the answers

Why is the potassium cation smaller than the potassium atom?

<p>Potassium cation has lost an electron and one energy level. (C)</p> Signup and view all the answers

What trend does ionization energy follow in the periodic table?

<p>Ionization energy generally increases across a period from left to right. (D)</p> Signup and view all the answers

Why does strontium have a smaller ionization energy compared to magnesium?

<p>Strontium has more energy levels, making it easier to remove an electron. (A)</p> Signup and view all the answers

What contributes to bromine having a larger ionization energy than calcium?

<p>Bromine has a stronger nuclear charge and is smaller. (B)</p> Signup and view all the answers

Which element in Group IIIA (3A) has the largest atomic radius?

<p>Indium (B)</p> Signup and view all the answers

Which scientist is credited with arranging elements by atomic number?

<p>Moseley (D)</p> Signup and view all the answers

Flashcards

Aufbau Principle

Fill lower energy electron orbitals first when writing electron configurations.

Pauli Exclusion Principle

Each electron has unique spin. Only two electrons can occupy one orbital, and they must have opposite spins.

Hund's Rule

Each orbital in a sublevel gets one electron before any gets two.

Electron Configuration

A notation describing the arrangement of all the electrons in an atom or ion.

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Valence Shell

The outermost electron shell of an atom.

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Valence Electrons

Electrons in the atom's outermost shell.

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Electron Orbital

A region in an atom where an electron resides.

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Noble Gas Notation

Short-hand way to write electron configurations, using a noble gas to represent the inner electrons.

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Atomic Number

The number of protons in an atom

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Sublevel

A division of electron orbitals with similar energy.

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Noble Gas Configuration

A shorthand notation for writing electron configurations, which uses the symbol of a noble gas to represent the core electrons and then adds the configuration of the remaining electrons.

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Shorthand Electron Configuration

A condensed representation of the electron configuration that uses the previous noble gas's configuration to represent the core electrons

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Aluminum's Noble Gas Configuration

[Ne]3s23p1

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Arsenic's Noble Gas Configuration

[Ar]4s23d104p3

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Calcium's Noble Gas Configuration

[Ar]4s2

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Phosphorus's Noble Gas Configuration

[Ne]3s23p3

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Zinc's Noble Gas Configuration

[Ar]4s23d10

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Metal Conductivity

Metals are good conductors of heat and electricity.

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Metalloid Properties

Metalloids have properties of both metals and nonmetals.

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Nonmetal Conductivity

Nonmetals are generally poor conductors of heat and electricity.

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Metal Luster

Metals typically have a shiny appearance.

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Metal State

Most metals are solids at room temperature, except mercury, which is liquid.

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Metal Ductility

Metals can be drawn into thin wires.

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Metal Malleability

Metals can be hammered or bent into different shapes without breaking.

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Nonmetal Brittleness

Nonmetals are often brittle and break easily.

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Shielding Effect

The reduction of the attraction between the nucleus and valence electrons by inner electrons.

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Effective Nuclear Charge (Zeff)

The net positive charge experienced by an electron in a multi-electron atom, considering the shielding effect of inner electrons.

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What happens to Zeff as you move down a group?

Zeff decreases as you move down a group because the number of inner electrons increases, resulting in greater shielding.

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Atomic Radius

The distance between the nuclei of two identical atoms bonded together.

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Ionization Energy

The minimum energy required to remove an electron from a gaseous atom in its ground state.

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Electronegativity

The ability of an atom to attract electrons within a chemical bond.

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Electron Affinity

The energy change when an electron is added to a neutral gaseous atom.

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Trends - Atomic Radius & Ionization Energy

Larger atomic radius corresponds to lower ionization energy, meaning it's easier to remove an electron from larger atoms.

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What is the Aufbau principle?

The Aufbau principle states that electrons fill the lowest energy levels first when writing electron configurations. This means that electrons will first occupy the 1s orbital before filling the 2s orbital, and so on.

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What is Hund's rule?

Hund's rule states that each orbital within a sublevel will receive one electron before any orbital receives two electrons. Electrons prefer to occupy separate orbitals with the same spin.

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What is Pauli's Exclusion Principle?

Pauli's Exclusion principle states that no two electrons in the same atom can have the same set of four quantum numbers. This practically means that an orbital can hold a maximum of two electrons, and they must have opposite spins.

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Why does atomic radius increase down a group?

Atomic radius increases down a group because the number of electron shells increases. This means the outermost electron is farther from the nucleus, making the atom larger.

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Why does atomic radius decrease across a period?

Atomic radius decreases across a period due to increasing effective nuclear charge. With each added proton, the nucleus pulls the electrons in more strongly, shrinking the atomic size.

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What are alkali metals?

Alkali metals are highly reactive, soft metallic solids. They have a silvery-white appearance, are good conductors of heat and electricity, and have low melting and boiling points. They are found in Group 1 of the Periodic Table.

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What are halogens?

Halogens are highly reactive, nonmetals. They exist in all states of matter at room temperature. Their melting and boiling points increase with increasing atomic number. They are found in Group 17 of the Periodic Table.

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What are noble gases?

Noble gases are colorless, odorless, tasteless, and inert gases. They are found in Group 18 of the Periodic Table.

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Atomic Radius Trend

The size of an atom generally increases as you move down a group and decreases as you move across a period. This is because the number of energy levels increases down a group, while the attraction between the nucleus and the electrons increases across a period.

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Ionization Energy Trend

Ionization energy, the energy required to remove an electron, generally increases as you move across a period and decreases as you move down a group. This is because the attraction between the nucleus and the electrons is stronger across a period.

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Why is Calcium larger than Bromine?

Calcium has a larger atomic radius than Bromine because Calcium has less effective nuclear charge pulling its outermost electrons closer to the nucleus. Bromine has a smaller atomic radius due to its stronger attraction between its nucleus and electrons.

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Why is Sulfide larger than Sulfur?

Sulfide, S⁻², is larger than Sulfur, S, because it has gained two electrons. This increases electron-electron repulsion, expanding the electron cloud.

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Why is Potassium cation smaller than Potassium atom?

Potassium cation (K⁺) is smaller than Potassium atom (K) because it has lost an electron resulting in a decrease in electron-electron repulsion and a stronger effective nuclear charge, pulling the remaining electrons closer to the nucleus.

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Why does Strontium have a smaller ionization energy than Magnesium?

Strontium has a larger atomic radius than Magnesium, making it easier to remove an electron. The electron is further away from the nucleus, experiencing weaker electrostatic attraction.

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Why does Bromine have a larger ionization energy than Calcium?

Bromine has a smaller atomic radius than Calcium, making it more difficult to remove an electron. The electron is closer to the nucleus and experiences a stronger electrostatic attraction.

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Who developed the Periodic Table?

Dmitri Mendeleev is credited with creating the first periodic table. He arranged elements in order of increasing atomic mass and left gaps for undiscovered elements, predicting their properties.

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Study Notes

Honors Unit 3: The Electron and Periodic Table

  • The periodic table displays elements arranged by atomic number.
  • Elements with similar properties are grouped together.
  • Rows on the table are called periods.
  • Columns on the table are called families or groups.
  • Atomic Models evolved over time with discoveries like the electron and nucleus.
  • Dalton's model, Thomson's model, Rutherford's model, Bohr Model, and the Quantum Mechanical model each expanded on previous understanding.
  • Atoms contain a nucleus with protons and neutrons, and electrons orbit the nucleus.
  • Electrons can gain or lose energy levels.
  • Light has wave properties, including amplitude and frequency, and wavelength.
  • Frequency and wavelength are inversely proportional. A shorter wavelength implies a higher frequency.
  • Elements emit light of specific wavelengths when heated. This is due to electrons switching energy levels.
  • The atomic emission spectrum is unique to each element.
  • Atomic orbitals are regions of space where electrons are likely found.
  • Orbitals have different shapes and orientations (s, p, d, f). Different orbitals hold various numbers of electrons.
  • Electron configuration describes the arrangement of electrons in orbitals within an atom.
  • Electron configuration follows the Aufbau Principle (filling lowest energy orbitals first), Hund's Rule (one electron in each orbital before doubling up), and Pauli Exclusion Principle (no two electrons have the same four quantum numbers).
  • Each electron can be represented by a coefficient (energy level), letter (orbital), and superscript (number of electrons).
  • Noble Gas notation is a shorthand representation of electron configuration.
  • Periods represent energy levels and groups represent valence electron similarities.
  • Periodic trends relate to properties like atomic radius, ionization energy, electronegativity, and electron affinity across the periodic table and within groups. These trends can be explained by changes in nuclear charge and shielding. An increase in nuclear charge results in a stronger attraction between the nucleus and electrons in an atom. Effective nuclear charge also affects the size of atoms.
  • Cations are positively charged ions (loss of electrons) while anions are negatively charged ions (gaining of electrons).
  • The size of ions differs from the size of parent atoms, depending on the gain or loss of electrons.

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Honors Unit 3: The Electron and Periodic Table Packet PDF

Description

This quiz covers the fundamental concepts of the electron, atomic models, and the organization of the periodic table. Explore how atomic theory evolved through various models, the arrangement of elements by atomic number, and the properties of light associated with atomic emission. Test your understanding of these key principles in chemistry.

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