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What happens to the first ionisation energy as you move across a period?
What happens to the first ionisation energy as you move across a period?
The first ionisation energy increases down a group.
The first ionisation energy increases down a group.
False
What is the effect of increasing atomic radius on first ionisation energy?
What is the effect of increasing atomic radius on first ionisation energy?
It decreases first ionisation energy.
The first ionisation energy __________ down groups due to increasing __________ and __________.
The first ionisation energy __________ down groups due to increasing __________ and __________.
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Match the following factors with their effects on first ionisation energy:
Match the following factors with their effects on first ionisation energy:
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Between lithium and carbon, which will have a lower first ionisation energy?
Between lithium and carbon, which will have a lower first ionisation energy?
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Beryllium has a lower first ionisation energy than magnesium.
Beryllium has a lower first ionisation energy than magnesium.
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Explain why magnesium has a lower first ionisation energy compared to beryllium.
Explain why magnesium has a lower first ionisation energy compared to beryllium.
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What is the atomic number of helium isotopes?
What is the atomic number of helium isotopes?
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Titanium has a higher percentage abundance of the isotope 48Ti than 47Ti.
Titanium has a higher percentage abundance of the isotope 48Ti than 47Ti.
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What percentage of naturally occurring carbon consists of carbon-13?
What percentage of naturally occurring carbon consists of carbon-13?
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The isotope ____Ti has the highest abundance among stable titanium isotopes.
The isotope ____Ti has the highest abundance among stable titanium isotopes.
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Match the following isotopes of titanium with their percentage abundance:
Match the following isotopes of titanium with their percentage abundance:
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How do scientists utilize atomic emission spectra?
How do scientists utilize atomic emission spectra?
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Carbon-12 and carbon-13 are both isotopes of carbon that can be detected by mass spectrometry.
Carbon-12 and carbon-13 are both isotopes of carbon that can be detected by mass spectrometry.
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Calculate the number of atoms of hydrogen in 16g of sulphuric acid (H2SO4).
Calculate the number of atoms of hydrogen in 16g of sulphuric acid (H2SO4).
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How many oxygen atoms are in one mole of oxygen gas?
How many oxygen atoms are in one mole of oxygen gas?
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Why is the 'M+1' peak visible but the 'M+2' peak not visible in the mass spectrum of a molecule consisting of two carbon atoms?
Why is the 'M+1' peak visible but the 'M+2' peak not visible in the mass spectrum of a molecule consisting of two carbon atoms?
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The empirical formula is the simplest whole number ratio of ______ in a compound.
The empirical formula is the simplest whole number ratio of ______ in a compound.
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The empirical formula of a compound with 23.3% magnesium, 30.7% sulphur, and 46.0% oxygen is MgSO4.
The empirical formula of a compound with 23.3% magnesium, 30.7% sulphur, and 46.0% oxygen is MgSO4.
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What is the empirical formula of a compound containing 60.0% sulphur and 40.0% oxygen by mass?
What is the empirical formula of a compound containing 60.0% sulphur and 40.0% oxygen by mass?
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Match the following compounds with their empirical formulas:
Match the following compounds with their empirical formulas:
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What is the molar mass of sulphuric acid (H2SO4)?
What is the molar mass of sulphuric acid (H2SO4)?
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The empirical formula of a compound can be the same as its molecular formula.
The empirical formula of a compound can be the same as its molecular formula.
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What primarily contributes to the high melting points of metallic structures?
What primarily contributes to the high melting points of metallic structures?
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Metallic structures are poor conductors of electricity.
Metallic structures are poor conductors of electricity.
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What term describes the attraction between positively charged metal ions and delocalised electrons?
What term describes the attraction between positively charged metal ions and delocalised electrons?
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A high amount of ___________________ is required to break the bonds in metallic structures.
A high amount of ___________________ is required to break the bonds in metallic structures.
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Match the property of metallic structures with its explanation:
Match the property of metallic structures with its explanation:
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What happens to the strength of a metallic bond as the charge of the metal ion increases?
What happens to the strength of a metallic bond as the charge of the metal ion increases?
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Metallic structures can conduct electricity when the ions are fixed in a lattice.
Metallic structures can conduct electricity when the ions are fixed in a lattice.
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What is required for metallic structures to conduct electricity?
What is required for metallic structures to conduct electricity?
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What is the resulting compound when tin (Sn) reacts with iodine (I2)?
What is the resulting compound when tin (Sn) reacts with iodine (I2)?
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When 5.00 g of hydrated tin (II) chloride are heated, the mass of the anhydrous compound formed is greater than 5.00 g.
When 5.00 g of hydrated tin (II) chloride are heated, the mass of the anhydrous compound formed is greater than 5.00 g.
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If 4.20 g of anhydrous tin (II) chloride is formed, how much water was lost during the heating of 5.00 g of hydrated tin (II) chloride?
If 4.20 g of anhydrous tin (II) chloride is formed, how much water was lost during the heating of 5.00 g of hydrated tin (II) chloride?
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The formula for the hydrated tin (II) chloride is SnCl2.xH2O, where x represents the number of molecules of ______.
The formula for the hydrated tin (II) chloride is SnCl2.xH2O, where x represents the number of molecules of ______.
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To calculate the percentage composition of carbon in a compound, which of the following must be known?
To calculate the percentage composition of carbon in a compound, which of the following must be known?
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Match the following compounds with their components:
Match the following compounds with their components:
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What is the total percentage mass of oxygen in a compound containing 2.20 g of hydrogen, 7.20 g of carbon, and 17.6 g of oxygen?
What is the total percentage mass of oxygen in a compound containing 2.20 g of hydrogen, 7.20 g of carbon, and 17.6 g of oxygen?
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The molar mass of SnCl2 is ______ g/mol.
The molar mass of SnCl2 is ______ g/mol.
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What is the formula to calculate percentage yield?
What is the formula to calculate percentage yield?
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The combustion of carbon disulfide produces only carbon dioxide as a product.
The combustion of carbon disulfide produces only carbon dioxide as a product.
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What are the products of burning carbon disulfide in the presence of oxygen?
What are the products of burning carbon disulfide in the presence of oxygen?
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The percent yield of a reaction can be calculated using the formula: __________.
The percent yield of a reaction can be calculated using the formula: __________.
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Match the compounds with their yields in the reaction of carbon disulfide combustion:
Match the compounds with their yields in the reaction of carbon disulfide combustion:
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If 25.0 g of carbon disulfide is burned and produces 40.5 g of sulfur dioxide, what contributes to the percent yield being less than 100%?
If 25.0 g of carbon disulfide is burned and produces 40.5 g of sulfur dioxide, what contributes to the percent yield being less than 100%?
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The theoretical yield of a reaction can always be achieved in practice.
The theoretical yield of a reaction can always be achieved in practice.
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Calculate the percentage yield if the actual yield of chlorobenzene is 63.7 g and the theoretical yield is 70 g.
Calculate the percentage yield if the actual yield of chlorobenzene is 63.7 g and the theoretical yield is 70 g.
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Study Notes
A Level OCR B Salters H033 Chemistry Booklet: Elements of Life Pt1
- Table of Contents: Provides a detailed outline of the topics covered in the booklet, with page numbers for each. Includes learning sequences, powerful knowledge sections, and practice exercises.
Data Sheet
- General Information: Includes key constants like Avogadro's constant, molar gas volume, specific heat capacity of water, Planck constant and more.
- Amino Acid Codons: Lists the triplet base codes (codons) for various amino acids used in mRNA.
Common lons
- Ion Formulae and Names: Provides a table listing common ion formulae alongside their respective names. (e.g., NO₃⁻-Nitrate, SO₄²⁻-Sulphate, CO₃²⁻-Carbonate, etc.)
Learning Sequence 1: Formulae and Equations
- Outcomes: Students will describe atomic structure and isotopes, explain mass spectrometry, and apply Avogadro's number to chemical calculations.
- Powerful Knowledge: Atomic Structure: Atoms consist of protons, neutrons and electrons located in different parts of the atom, with unique masses and charges. The nucleus holds protons and neutrons, while the electron cloud surrounds the nucleus.
- Atomic Number: The atomic number represents the number of protons in an atom of an element.
- Mass Number (Relative Atomic Mass): The sum of protons and neutrons in an atom.
- Isotopes: Atoms of the same element (same number of protons) that have different numbers of neutrons.
- Mass Spectrometry: Used to determine the abundance of isotopes.
Powerful knowledge: Isotopes
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Isotope Definition: Atoms of the same element with different numbers of neutrons, hence, different mass numbers. Their chemical behavior is the same due to identical electron numbers.
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Calculating isotopic elements: Various exercises to calculate relative atomic mass from isotopic data.
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Example: Carbon (C) has isotopes 12C, 13C and 14C all having the same number of protons but different numbers of neutrons.
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Powerful knowledge: Mass spectroscopy Explains how mass spectrometers work by vaporizing, ionizing, accelerating, deflecting, and detecting ions to determine the mass-to-charge ratio (m/z) and abundance of each isotope.
Powerful knowledge: Calculating Average Atomic Mass of Isotopes
- Method: Weighted average based on isotopic masses and natural abundances.
- Formula: Utilizes the formula to calculate average atomic mass from isotopic masses and abundances.
Learning Sequence 3: Bonding and Structure
- Outcomes: Students describe covalent and dative bonding in molecules, describe ionic and metallic bonding using ideas about ions, and describe the properties of simple molecular, massive covalent, ionic lattice and metallic structures.
Powerful knowledge: Covalent Bonding
- Definition: Atoms share one or more pairs of electrons to reach a stable electron configuration, usually observed between nonmetals.
Dative Covalent Bonds
- Definition: One atom provides both electrons to be shared in the covalent bond, typically with one atom having a lone pair electron and the other having an empty orbital.
Powerful knowledge: Ionic Bonding
- Definition: Electrons are transferred or shared creating ions for achieving stability. Characteristic of metals binding with nonmetals.
Powerful knowledge: Metallic Bonding
- Definition: Lattice formed by positive ions in a sea of delocalized electrons.
Powerful knowledge: Structure and Properties of Simple Molecular Structures
- Structures and Properties: Simple molecular structures have low melting and boiling points and poor conductivity due to weak intermolecular forces holding the molecules together. They generally consist of non-metallic elements.
Powerful knowledge: Structure and Properties of Giant Covalent Structures
- Structure and Properties: Examples like diamond and graphite are good examples of such structures characterized by extremely strong covalent bonds, which lead to high melting and boiling points. They may or may not conduct electricity, depending on the structure.
Powerful knowledge: Structure and Properties of Ionic Compounds
- Structure and Properties: Giant ionic lattices are formed between metallic and nonmetallic elements with ions forming a crystal lattice structure causing high melting and boiling points due to strong electrostatic interactions. Generally poor conductors of electricity in their solid state but can conduct in molten or dissolved form.
Powerful knowledge: Structure and Properties of Metallic Structures
- Structure and Properties: Consist of metallic ions surrounded by a sea of delocalized electrons. Metallic structures have high melting and boiling points and are good conductors of both electricity and heat. The ability to conduct is caused by the mobility of electrons.
Learning Sequence 4: Amount of Substances and Chemical Calculations
- Outcomes: Students define the mole, calculate moles in mass, calculate reacting masses, and perform percentage yield and composition calculations.
- Powerful knowledge: Number of Moles: One mole of any substance contains Avogadro's number of entities (atoms, molecules, etc.).
- Molar Calculations: Calculates reacting mass, amount of product formed, or needed reactants. Utilize stoichiometric ratios from balanced chemical equations.
- Percentage yield: Compares actual yield (amount experimentally obtained) to theoretical yield (calculated yield). Provides an insight into the efficiency of a reaction.
Powerful knowledge: Percentage Composition
- Definition: Percentage composition describes the percentage of each element by mass in a compound. Using molar mass and the percentage composition enables calculation of the empirical formula
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Description
Test your understanding of first ionisation energy trends and isotopic abundance in this quiz. Explore how atomic radius and group positioning affect ionisation energy, along with the significance of atomic emission spectra. This quiz covers essential concepts in chemistry.
