knowverseIonic vs covalent bonds: which one is each statement about?
In an ionic bond one atom takes an electron from the other and the two ions attract; in a covalent bond two atoms share a pair of electrons. This page lets you sort ten statements about ionic vs covalent bonds, then shows the answers and a table of key differences.
After the sorting game you will find a concise comparison table that lists how electrons move, the role of electronegativity difference, typical partners, the structures formed, overall charge, and everyday examples such as table salt and water and methane for reference.
Key differences between ionic and covalent bonds
| Aspect | Ionic | Covalent |
|---|---|---|
| Electrons | Transferred: one atom takes an electron from the other | Shared: both nuclei pull on the same pair of electrons |
| Electronegativity | Needs a large difference between the two atoms | Similar or equal pull, often two nonmetals |
| Typical partners | Atoms like sodium and chlorine | Two nonmetals, such as carbon, oxygen or nitrogen |
| What forms | A repeating crystal lattice of ions | Distinct molecules, like water (H2O) or methane (CH4) |
| Charge | Positive and negative ions held by electrostatic attraction | The molecule stays electrically neutral overall |
| Everyday example | Table salt (NaCl) | Water, methane, hydrogen gas |
Ionic vs covalent bonds: sort the statements
Sort each statement: does it describe Ionic or Covalent? The answers stay hidden until you check them all.
- Statement 1
One atom takes an electron from the other, and the two charged atoms pull together.
It describes Ionic
The passage explains that an electron is taken from one atom, producing a positive ion and a negative ion that attract each other. This attraction builds a repeating lattice rather than isolated molecules. The lattice structure is why solid salts are hard and brittle.
Source excerpt
In summary, an ionic bond is the result of an electron 'theft' that creates oppositely charged ions, which then pull together into a lattice.
From the Knowverse course text.
- Statement 2
Both nuclei pull on the same pair of electrons at the same time.
It describes Covalent
The text notes that both nuclei pull on the same electron pair at the same time, which is the hallmark of sharing rather than transfer. This shared pair holds the atoms together in a discrete molecule. The shared electrons keep the overall unit electrically neutral.
Source excerpt
Instead of a transfer, the two nuclei begin to pull on the same pair of electrons simultaneously.
From the Knowverse course text.
- Statement 3
It usually forms between two nonmetals, such as carbon, oxygen or nitrogen.
It describes Covalent
The passage states that this bonding typically forms between two nonmetals like carbon, oxygen, or nitrogen. Because both atoms have high electronegativity, neither readily gives up an electron. The result is a molecule such as water or methane rather than a crystal lattice.
Source excerpt
This type of bonding usually occurs between two nonmetals, such as Carbon, Oxygen, or Nitrogen.
From the Knowverse course text.
- Statement 4
It needs a large difference in electronegativity between the two atoms.
It describes Ionic
The evidence says a large electronegativity difference is needed for this bond type; without it, both atoms would try to lose electrons and no anion would form. This requirement explains why metals pair with nonmetals. The difference drives the electron transfer that creates ions.
Source excerpt
Ionic bonds require a large difference in electronegativity. Two sodium atoms both want to lose electrons, so there is no 'receiver' to take the electron and form an anion.
From the Knowverse course text.
- Statement 5
It is held together by the attraction between a positive and a negative ion.
It describes Ionic
The passage describes how electron loss or gain creates charged ions that attract each other electrostatically. This attraction holds the ions in a rigid lattice. The lattice breaks cleanly when struck because like charges align and repel. This brittleness is a hallmark of ionic solids.
Source excerpt
By losing or gaining an electron, the atoms are no longer neutral; they have become ions. Because one is positive and the other is negative, they experience a powerful electrostatic attraction.
From the Knowverse course text.
- Statement 6
It makes distinct molecules, such as water and methane.
It describes Covalent
The text points out that sharing electrons yields separate molecules such as water and methane. These molecules stay intact in the solid, liquid, or gas phase. Unlike a lattice, each molecule keeps its own identity. This molecular nature explains low melting points.
Source excerpt
Because covalent bonds create distinct molecules, we can have substances like water (H2O) or methane (CH4).
From the Knowverse course text.
- Statement 7
The solid does not conduct electricity, but the melted compound does.
It describes Ionic
The passage explains that in the solid state ions cannot move, so no current flows. Melting frees the ions to carry charge. This is why molten salt conducts electricity while solid salt does not. The change from fixed to mobile ions is the key.
Source excerpt
While solid ionic compounds are insulators because the ions are locked in the lattice, melting them allows the ions to move freely. These mobile charges can then carry an electric current.
From the Knowverse course text.
- Statement 8
Two atoms can share two or even three pairs of electrons, making double and triple bonds.
It describes Covalent
The evidence notes that atoms may share two or three electron pairs, forming double or triple bonds. This multiplicity is unique to covalent bonding. Multiple shared pairs shorten the distance between nuclei and increase bond strength. These stronger bonds affect molecular geometry.
Source excerpt
While this chapter focused on single pairs, atoms can share two or even three pairs of electrons to reach their octet. These are called double and triple bonds, which we will explore in an upcoming chapter.
From the Knowverse course text.
- Statement 9
Its crystals shatter when hit, because like charges suddenly line up and repel.
It describes Ionic
The passage links the rigid lattice to brittleness: a blow shifts layers so that like charges line up and repel. This repulsion causes the crystal to fracture cleanly. The same electrostatic forces that hold the lattice also make it fragile.
Source excerpt
This rigid structure also explains why salt crystals shatter when hit; the layers shift, and like-charges suddenly repel each other.
From the Knowverse course text.
- Statement 10
The bonded unit stays electrically neutral overall, with no ions formed.
It describes Covalent
The text states that the molecule keeps equal numbers of protons and electrons, so it stays neutral overall. No ions are formed, unlike in ionic compounds where charges separate. This neutrality means covalent substances do not conduct electricity in any state.
Source excerpt
Because the total number of protons in the nuclei still equals the total number of electrons in the molecule, the overall unit remains electrically neutral. This is a big difference from ionic compounds.
From the Knowverse course text.
Questions people ask
Is table salt (NaCl) ionic or covalent?
Table salt (NaCl) is an ionic compound because sodium transfers an electron to chlorine, forming a lattice of oppositely charged ions. This structure makes solid salt an insulator until melted.
Can a bond be partly ionic and partly covalent?
The course notes that a large difference favors ionic bonding while a small difference favors covalent sharing; an intermediate gap gives a bond with mixed character. Such bonds are common in compounds like hydrogen chloride.
Why do ionic compounds conduct electricity only when melted?
Solid ionic compounds are insulators because the ions cannot move; when melted the ions become mobile and can conduct an electric current. This change from fixed to mobile ions explains the conductivity shift.
If you want to master bonding step by step, the Knowverse course Principles of Chemical Bonding guides you through electron transfer, sharing, electronegativity, and lattice versus molecule behavior with clear lessons and practice. Each module builds on the last so you gain confidence before moving on.
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Sources: Principles of Chemical Bonding. Each statement is settled by an excerpt from the course.