2.2 How bonding and structure are related to the properties of substances

Cards (139)

Ionic bonding involves the electrostatic attraction between oppositely charged ions
Metals have low ionization energy. 
True
What type of bonding is present in a methane molecule (CH4)?
Covalent
Covalent compounds have high melting and boiling points.
False
Match the bonding type with an example substance:
Ionic ↔️ NaCl
Covalent ↔️ H2
Metallic ↔️ Cu
Metallic bonding enables high malleability and conductivity. 
True
Covalent bonding occurs when atoms share electrons
In covalent bonding, atoms share electrons
Match the type of bonding with the atoms involved:
Ionic ↔️ Metal and non-metal
Covalent ↔️ Non-metals
What is the bond strength of covalent bonds compared to ionic bonds?
Strong
Covalent compounds have poor conductivity
What is metallic bonding characterized by?
Delocalized electrons
Metallic bonding has a strong bond strength
Ionic compounds conduct electricity when dissolved
A hydrogen molecule (H2) consists of two hydrogen atoms sharing a pair of electrons. 
True
Why do covalent compounds have poor electrical conductivity compared to ionic and metallic compounds?
No free electrons
Match the type of atom with its electron behavior in ionic bonding:
Metals ↔️ Lose electrons
Non-metals ↔️ Gain electrons
What type of electronegativity differences lead to covalent bonding?
Similar
What type of bond is formed in a hydrogen molecule (H2)?
Covalent
Match the property with the type of bonding:
Complete electron transfer ↔️ Ionic bonding
Shared electrons ↔️ Covalent bonding
Ionic compounds typically have high melting and boiling points due to strong electrostatic attractions
What is the key characteristic of metallic bonding?
Delocalized electrons
Rank the electrical conductivity of bonding types from highest to lowest:
1️⃣ Metallic bonding
2️⃣ Ionic bonding (in solution)
3️⃣ Covalent bonding
What is the structure of ionic compounds?
Lattice of ions
Sodium chloride (NaCl) forms a cubic lattice
What type of bonding is present in methane (CH4)?
Covalent
Metallic bonding results in high electrical conductivity due to delocalized electrons.
True
Why do ionic compounds have high melting and boiling points?
Strong electrostatic forces
When dissolved in water, ionic compounds become good conductors of electricity.
True
Covalent substances have properties such as low melting and boiling points, poor electrical conductivity, and varying solubility
Match the property with the type of covalent structure:
Melting/Boiling Points ↔️ Low for simple molecules, High for giant structures
Electrical Conductivity ↔️ Poor for both types
Solubility ↔️ Variable for simple molecules, Insoluble for giant structures
Covalent bonding occurs when atoms have similar electronegativities and share pairs of electrons
Ionic bonding involves the sharing of electrons between non-metal atoms.
False
Arrange the following steps in the formation of an ionic lattice:
1️⃣ Positive ions (cations) are formed
2️⃣ Negative ions (anions) are formed
3️⃣ Electrostatic attraction between ions
4️⃣ Ions arrange in a regular lattice
What type of bond is formed when hydrogen atoms share a pair of electrons?
Covalent bond
What is the structure of covalent compounds?
Molecules
Covalent compounds have variable melting and boiling points
What is shared in metallic bonding?
Delocalized electrons
Metallic substances are good conductors of electricity.
True
Ionic compounds do not conduct electricity in their solid form because the ions are tightly bound.