Atomic Structure and Periodic Table
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Questions and Answers

What is the peak with the largest m/z value in mass spectrometry called?

  • Base peak
  • Isotope peak
  • Fragment ion
  • Parent ion (correct)

Mass spectrometers can be used for radioactive dating.

True (A)

What is the first ionisation energy?

The energy required when one mole of gaseous atoms forms one mole of gaseous ions with a single positive charge.

The equation for first ionisation energy can be represented as H(g) → H+ (g) + ______

<p>e-</p> Signup and view all the answers

Match the following applications of mass spectrometers with their uses:

<p>Planetary space probes = Identify elements on other planets Drug testing = Identify chemicals and breakdown products in the blood Quality control = Ensure pharmaceutical products meet standards Radioactive dating = Determine age of fossils or human remains</p> Signup and view all the answers

Which of the following is not a use of mass spectrometers?

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

The molecular ion peak is always the most abundant peak in a mass spectrum.

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

What does the m/z value represent in mass spectrometry?

<p>Mass-to-charge ratio.</p> Signup and view all the answers

What type of bonding is primarily found in silicon (Si)?

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

S8 has a higher melting point than P4 due to stronger London forces.

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

What is the primary reason for the low melting and boiling points of Cl2?

<p>Weak London forces</p> Signup and view all the answers

The melting point of S8 is influenced by the number of _____ it has compared to P4.

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

Match the following substances with their correct properties:

<p>Na = Metallic bonding with high melting point N2 = Molecular gas with low melting point Ar = Monoatomic gas with weak London forces C = Macromolecular with very high melting point</p> Signup and view all the answers

What is the definition of second ionisation energy?

<p>Energy required when one mole of gaseous ions with a single positive charge forms one mole of gaseous ions with a double positive charge (D)</p> Signup and view all the answers

The first ionisation energy is always larger than the second ionisation energy for an element.

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

What happens to the attraction experienced by the remaining electrons after the removal of the first electron?

<p>The attraction increases.</p> Signup and view all the answers

The larger the atom, the further the outer electrons are from the nucleus, resulting in _______ attraction.

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

Match the factors affecting ionisation energy with their descriptions:

<p>Attraction of the nucleus = Greater protons lead to stronger attraction Distance of the electrons = Outer electrons feel less attraction if farther away Shielding effect = Inner shell electrons repel the outer shell electrons</p> Signup and view all the answers

What represents the process of second ionisation energy in a chemical equation?

<p>Ti+(g) → Ti2+(g) + e- (A)</p> Signup and view all the answers

Shielding refers to the effect of outer electrons on the inner electrons of an atom.

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

Explain why successive ionisation energies become larger.

<p>Because the positive charge increases, leading to greater attraction on remaining electrons.</p> Signup and view all the answers

What does a large jump in ionisation energy indicate about an element's group placement?

<p>It must be in group 2. (C)</p> Signup and view all the answers

The ionisation energy of an element increases as more electrons are removed from the outer shell.

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

What group of the periodic table does the element belong to if there is a significant increase between the 2nd and 3rd ionisation energies?

<p>Group 2</p> Signup and view all the answers

The first ionisation energy of helium is _____ compared to other elements.

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

Match the following terms with their descriptions:

<p>Ionisation Energy = Energy required to remove an electron Periodicity = Repeating pattern across a period Effective Nuclear Charge = Net positive charge experienced by an electron Shell = Energy level where electrons reside</p> Signup and view all the answers

Which factor contributes to the increased ionisation energy when removing the third electron?

<p>Decreased distance from the nucleus (A)</p> Signup and view all the answers

The shape of the graph for ionisation energies across periods two and three is different.

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

Why does helium have the largest first ionisation energy?

<p>It has a full outer shell.</p> Signup and view all the answers

What does the relative atomic mass represent?

<p>A weighted average of all isotopes (C)</p> Signup and view all the answers

The m/z value for a 24Mg2+ ion is 12.

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

What formula is used to calculate the relative atomic mass (R.A.M)?

<p>R.A.M = Σ (isotopic mass x % abundance) / total relative abundance</p> Signup and view all the answers

The isotopes of chlorine are Cl35 and Cl37, with percentages of __________ and __________, respectively.

<p>75%, 25%</p> Signup and view all the answers

Match the isotopes with their respective abundances.

<p>Cl35 = 75% Cl37 = 25% Br79 = 50% Br81 = 50%</p> Signup and view all the answers

Which of the following is true regarding mass spectra?

<p>Peaks may correspond to fragments from the same molecule. (C)</p> Signup and view all the answers

Relative atomic mass calculations require the total number of isotopes.

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

How are the m/z values in a mass spectrum calculated?

<p>m/z is calculated as the mass of the ion divided by its charge.</p> Signup and view all the answers

For the molecule C4H10, the mass spectrometer produces a spectrum that often includes __________ peaks due to fragmentation.

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

Match the isotopes with their elements.

<p>Cl35 = Chlorine Cl37 = Chlorine Br79 = Bromine Br81 = Bromine</p> Signup and view all the answers

What happens when the second electron is added to a 3p orbital?

<p>There is a slight repulsion between the two electrons. (C)</p> Signup and view all the answers

The second ionisation energy pattern is the same as the first, but shifted one to the right.

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

Which electron configuration represents phosphorus?

<p>1s2 2s2 2p6 3s2 3p3</p> Signup and view all the answers

Lithium's second ionisation energy is _____ than that of helium.

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

Match the element to its respective second ionisation energy trend:

<p>Li = High second ionisation energy Ne = Low second ionisation energy Na = Medium second ionisation energy Ar = Higher second ionisation energy</p> Signup and view all the answers

Which of the following elements has the second largest ionisation energy?

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

Sulfur has an electron configuration ending in 3p4.

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

In which shell is the second electron of lithium primarily found?

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

Flashcards

Relative Atomic Mass (RAM)

The average mass of an element's atoms, taking into account the relative abundance of its isotopes.

Isotopes

Different forms of an element that have the same number of protons but different numbers of neutrons.

Isotopic Abundance

The percentage of each isotope present in a naturally occurring sample of an element.

RAM Calculation Equation

The formula used to calculate the relative atomic mass of an element.

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Mass Spectrometry

A technique used to separate ions based on their mass-to-charge ratio (m/z).

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Mass Spectral Peak

A peak on a mass spectrum representing a specific ion with a unique mass-to-charge ratio.

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Mass-to-Charge Ratio (m/z)

The mass-to-charge ratio (m/z) of a molecule or ion in a mass spectrometer.

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Fragmentation

When molecules break apart into smaller fragments in a mass spectrometer.

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Mr

The relative molecular mass of a molecule.

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Mass Spectrum for a Molecule

A type of mass spectrum that provides information about the fragmentation pattern of a molecule.

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Molecular Ion Peak

The peak in a mass spectrum with the highest m/z value. It represents the intact molecule and its mass.

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Ionization

The process of removing an electron from a neutral atom, creating a positively charged ion.

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First Ionization Energy

The minimum amount of energy required to remove one electron from a mole of gaseous atoms, forming positive ions and electrons.

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Isotopic Composition

The specific arrangement of isotopes that make up an element, as found in a particular location.

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Radioactive Dating

The use of mass spectrometry to determine the age of ancient objects, like fossils, by analyzing the decay of radioactive isotopes.

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Molecular Identification

The process of identifying specific molecules in complex mixtures, such as analyzing blood or urine samples for drug testing.

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Pharmaceutical Applications

The use of mass spectrometry in the pharmaceutical industry to ensure product quality and identify new molecules with potential therapeutic properties.

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Second Ionisation Energy

The energy required to remove one mole of electrons from one mole of gaseous ions with a single positive charge, forming one mole of gaseous ions with a double positive charge.

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Third Ionisation Energy

The energy required to remove one mole of electrons from one mole of gaseous ions with a double positive charge, forming one mole of gaseous ions with a triple positive charge.

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Nuclear Attraction

The greater the attraction between the nucleus and the outermost electron, the more energy is required to remove it.

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Distance from Nucleus

The larger the atom, the further the outermost electron is from the nucleus, and the weaker the attraction.

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Shielding Effect

Electrons in inner shells shield outer electrons from the full nuclear attraction, making it easier to remove outer electrons.

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Trend in Ionisation Energies

Successive ionisation energies increase as more electrons are removed because the ion becomes increasingly smaller and more positively charged, leading to stronger attraction for the remaining electrons.

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Ionisation Energy Jumps

Large jumps in ionisation energies occur when an electron is removed from a stable, filled shell, indicating a significant increase in attraction for the remaining electrons.

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Ionisation Energy Trend (Across Period)

The energy required to remove electrons from an atom increases as you move across a period from left to right.

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Ionisation Energy Trend (Down Group)

The energy required to remove electrons from an atom decreases as you move down a group.

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Core Electron Shielding

Shells of electrons that are closer to the nucleus have a stronger attraction to the nucleus.

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Periodicity

The repeating pattern of properties observed across a period in the periodic table.

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Melting and boiling points are affected by bond strength

The strength of the bonds between atoms in a substance determines its melting point and boiling point. Stronger bonds require more energy to break, resulting in higher melting and boiling points.

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What are macromolecules?

Macromolecules are substances with many strong covalent bonds between atoms, leading to very high melting and boiling points. They require significant energy to break the bonds, making them solid at room temperature.

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What are simple molecular substances?

Simple molecular substances have weak intermolecular forces (London forces) between molecules. These forces easily break with minimal energy, resulting in low melting and boiling points. They exist as gases or liquids at room temperature.

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How does molecular size affect London forces?

The size of a molecule affects the strength of London forces. Larger molecules with more electrons have stronger London forces, leading to higher melting and boiling points.

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What are monoatomic substances?

Monoatomic substances like noble gases have very weak London forces between atoms. These forces are easily broken, resulting in extremely low melting and boiling points. They exist as gases at room temperature due to the minimal attraction between their atoms.

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Why does sulfur have a lower second ionisation energy than phosphorus?

The repulsion between two electrons in the same 3p orbital makes it easier to remove the second electron.

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Why do group 1 elements appear at the peaks of the 2nd Ionisation Energy graph?

The group 1 elements now appear at the peaks of the graph because their second electron is removed from the first electron shell, which is closer to the nucleus and experiences less shielding.

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Why does lithium have a higher second ionisation energy than helium?

Lithium has a bigger second ionisation energy than helium because lithium has more protons in its nucleus, leading to a stronger attraction between the nucleus and the remaining electron.

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Ionisation Energy

The energy needed to remove all the electrons from a neutral atom to form a cation.

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How does the distance between the nucleus and the electron affect ionization energy?

The closer an electron is to the nucleus, the stronger the attraction between the nucleus and the electron. This makes it harder to remove the electron.

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Study Notes

Atomic Structure and the Periodic Table

  • Atoms are composed of protons, neutrons, and electrons.
  • Protons have a positive charge, neutrons have no charge, and electrons have a negative charge.
  • Protons and neutrons are located in the nucleus, while electrons orbit the nucleus.
  • Atomic number (Z) represents the number of protons in an atom.
  • Mass number (A) is the total number of protons and neutrons.
  • Isotopes are atoms of the same element with different numbers of neutrons.
  • Relative isotopic mass compares the mass of an isotope to one-twelfth the mass of a carbon-12 atom.
  • Relative atomic mass is the weighted average mass of an atom compared to one-twelfth the mass of a carbon-12 atom.
  • Relative molecular mass is the average mass of a molecule compared to one-twelfth the mass of a carbon-12 atom.

Mass Spectrometer

  • Mass spectrometers determine the isotopes present in a sample.
  • They identify elements by measuring the mass-to-charge ratio (m/z) of ions.
  • Relative atomic mass is calculated as a weighted average of isotopic masses.
  • The spectrometer's output shows a spectrum with peaks corresponding to different isotopes.
  • Each peak represents an isotope, its abundance and its m/z value.

Ionization Energies

  • The first ionization energy is the minimum energy needed to remove one electron from each atom in a mole of gaseous atoms.
  • Successive ionization energies are progressively higher because removing electrons from a positively charged ion requires more energy.
  • Ionization energy trends: It tends to increase across a period due to increasing nuclear charge. It tends to decrease down a group due to increased electron shielding and larger atomic radius. There are occasional irregularities.
  • Factors affecting ionization energy: Effective nuclear charge, atomic radius and shielding.
  • The large jump between successive ionization energies indicates the removal of an electron from a different energy level. This can be used for identifying the electronic structure of an element.

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Atomic Structure and Periodic Table PDF - IGCSE

Description

Test your knowledge on atomic structure and the periodic table. This quiz covers the basics of protons, neutrons, electrons, isotopes, and mass spectrometry. Perfect for students studying chemistry concepts related to atomic theory and elemental identification.

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