Chemistry /Edexcel A Level Chemistry: 2: Bonding and Structure Part 1
Edexcel A Level Chemistry: 2: Bonding and Structure Part 1
This deck covers key concepts in ionic and covalent bonding, including the effects of ionic radius and charge, properties of ionic compounds, and the nature of covalent bonds. It also explores bond length, bond energy, and electronegativity.
What is ionic bonding?
The strong electrostatic attraction between oppositely charged ions
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Key Terms
Term
Definition
What is ionic bonding?
The strong electrostatic attraction between oppositely charged ions
What effects does ionic radius have on the strength of ionic bonding?
The smaller the radius, the stronger the ionic bond
What effects do charges have on ionic bonding?
The greater the charge, the stronger the bond
How are ions formed?
By the loss (+) or gain (-) of electrons
What is a cation?
A positively charged ion
What is an anion?
A negatively charged ion
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| Term | Definition |
|---|---|
What is ionic bonding? | The strong electrostatic attraction between oppositely charged ions |
What effects does ionic radius have on the strength of ionic bonding? | The smaller the radius, the stronger the ionic bond |
What effects do charges have on ionic bonding? | The greater the charge, the stronger the bond |
How are ions formed? | By the loss (+) or gain (-) of electrons |
What is a cation? | A positively charged ion |
What is an anion? | A negatively charged ion |
What does isoelectronic mean? | Two or more molecular entities that have the same number of electrons or a similar electron configuration |
How does a positive charge affect atomic radius? | It gets smaller because it loses electrons from its outer shell |
How does a negative charge affect ionic radius? | It gets larger because electrons are added to the outer shell |
What are the trends in atomic radii for ions with different charges? | The larger the charge, the bigger the change in the ion’s size |
How can the migration of ions be observed? | During electrolysis of coloured compounds |
What does ionic migration prove? | The existence of ions |
What are the melting/boiling temperatures of ionic compounds like? | They’re high due to the strong bonds |
What are ionic compounds like physically? | They’re hard, brittle, crystalline substances |
How soluble are ionic compounds? | They’re soluble in water and other polar solvents but insoluble in non-polar solvents |
Do ionic compounds conduct? | Not when solid, because their ions cannot move away from their fixed positions, but they do conduct when melted or dissolved |
What happens when ions reach the anode? | They lose electrons |
What happens when ions reach the cathode? | They gain electrons |
What is a covalent bond? | The strong electrostatic attraction between two nuclei and the shared pairs of electrons between them |
What is a dative covalent bond? | One in which both the electrons in the bonding pair are provided by one atom |
What do lone pairs of electrons do? |
|
What is bond length? | The distance between the nuclei of two bonded atoms in a molecule |
How can bond lengths be measured? | Using X-Ray diffraction when solid or Microwave spectroscopy when gaseous |
What does bond length depend on? | The size of atoms involved and the number of pairs of electrons shared |
Why do large atoms form longer bonds? | Because they have more electrons which shield the nuclei and reduce the attraction for the electron cloud. |
Single bonds are… | …longer than double bonds, which are longer than triple bonds |
Why are triple bonds shortest? | The nuclei can remain closer together if the shared electron cloud contains more electrons to overcome the repulsion of the nuclei |
What is bond energy? | The energy required to break one mole of the bonds in a substance in the gaseous state |
Which bonds have greater bond strength? | Single bonds, they’re stronger and have greater bond energy. |
What is the shape of a simple molecule or ion determined by? | The repulsion between the electron pairs that surround the central atom |
What is electronegativity? | The ability of an atom to attract the bonding electrons in a covalent bond |
Ionic and covalent bonds are the extremes of… | …a continuum of bonding type |
Electronegativity differences lead to… | …bond polarity in bonds and molecules |
What are the 3 most electronegative elements? | Nitrogen, Oxygen, Fluorine |
How do London Forces occur? | When non-polar atoms or molecules meet and there are fleeting repulsion and attractions between the nuclei of the atoms and surrounding clouds of electrons |