C3 Flashcards
(29 cards)
identify the three states of matter and
their state symbols
Solid(s) liquid(aq) gas
describe the process melting.
Melting occurs when the molecules of a solid speed up enough that the motion overcomes the attractions so that the molecules can move past each other as a liquid.
Process of freezing
Freezing is the process that causes a substance to change from a liquid to a solid. Freezing occurs when the molecules of a liquid slow down enough that their attractions cause them to arrange themselves into fixed positions as a solid.
state the particles involved in ionic bonding and examples
For ionic bonding the particles are oppositely charged ions. Examples:NaCl: sodium chloride.
NaBr: sodium bromide.
NaF: sodium fluoride.
NaI: sodium iodide.
KF: potassium fluoride.
state the particles involved in covalent bonding. And some examples
The sharing of electrons between atoms is called a covalent bond, which holds the atoms together as a molecule. A covalent bond happens if the attractions are strong enough in both atoms and if each atom has room for an electron in its outer energy level. Examples:water, carbon dioxide, ammonia, ozone, glucose,
describe, with an example, how a
Group 1 metal atom becomes a positive ion.
Group 1 metals form +1 ions because they have one electron in their outermost shell, which they lose to achieve a stable electron configuration. How lithuim can give a electron to a atom in group 0
describe, with an example, how a
Group 7 non-metal atom becomes a
negative ion.
It becomes a negative due to gaining an ion to complete it outer shell due to gaining an electron from group 1
explain, in terms of particles, energy
and temperature of a substance when it is
at the melting point
Melting Point: Particles gain energy, vibrate more, and overcome some forces of attraction, allowing them to move past each other as the solid turns into a liquid. Temperature remains constant during melting.
explain, in terms of particles, energy
and temperature of a substance when it is
at the boiling point.
Boiling Point: Particles absorb more energy, move faster, and break free from all forces of attraction, becoming a gas. Temperature remains constant during boiling.
describe the factors that affect rate
of evaporation.
Temperature – Higher temperature = faster evaporation (more particle energy).
Surface Area – Larger surface = faster evaporation (more particles exposed).
Humidity – Lower humidity = faster evaporation (less water vapor in air).
explain how electron transfer allows
ionic bonding to occur in the compound
formed when a Group 1 metal reacts with
a Group 7 non-metal.
A Group 1 metal loses 1 electron to form a positive ion (+1), while a Group 7 non-metal gains 1 electron to form a negative ion (-1). The opposite charges attract, creating a strong ionic bond.
suggest why substances have
different melting and boiling points from
each other.
Different substances have different bond strengths and forces between particles. Stronger bonds (e.g., ionic, covalent, metallic) or forces (e.g., intermolecular forces) require more energy to break, leading to higher melting and boiling points.
suggest and explain the charge of a
monatomic ion based on its position in the
periodic table.
Group 1: Loses 1 electron → +1 charge
Group 2: Loses 2 electrons → +2 charge
Group 6: Gains 2 electrons → -2 charge
Group 7: Gains 1 electron → -1 charge
state that opposite charges attract.
Opposite charge attracts
write the charges of ions of Group 1,
Group 2, Group 6, and Group 7 elements.
Group 1: +1
Group 2: +2
Group 6: -2
Group 7: -1
describe an ionic lattice.
An ionic lattice is a giant structure of oppositely charged ions arranged in a regular, repeating pattern. The strong electrostatic forces between the ions hold the structure together.
state that ionic compounds have high
melting points and can dissolve in water.
ionic compounds have high
melting points and can dissolve in water.
state that ionic compounds can
conduct electricity when molten or
dissolved in water.
ionic compounds can
conduct electricity when molten or
dissolved in water.
describe a covalent bond.
A covalent bond is a shared pair of electrons between two non-metal atoms, creating a strong bond that holds the atoms together.
name familiar examples of small
molecules which contain covalent bonds.
Water (H₂O), Oxygen (O₂), carbon dioxide
explain how the position of an
element on the periodic table relates to the
charge on its most stable monatomic ion.
The charge of an ion depends on how many electrons an atom loses or gains to get a full outer shell:
Group 1: +1 (loses 1 electron)
Group 2: +2 (loses 2 electrons)
Group 6: -2 (gains 2 electrons)
Group 7: -1 (gains 1 electron)
Metals lose electrons to form positive ions, while non-metals gain electrons to form negative ions.
explain, in terms of electronic
structure, how unfamiliar elements
become ions.
Atoms gain or lose electrons to get a full outer shell (like noble gases).
Metals lose electrons → form positive ions (cations)
Non-metals gain electrons → form negative ions (anions)
The number of electrons lost or gained depends on the element’s group in the periodic table.
explain why ionic compounds have
a high melting point.
Ionic compounds have strong electrostatic forces between oppositely charged ions in a lattice structure. These forces require a lot of energy to break, resulting in a high melting point.
describe, in terms of ions, how an
ionic compound can conduct electricity.
Ionic compounds can conduct electricity when they are molten or dissolved in water. This is because the ions are free to move and carry an electric charge. In a solid state, ions are fixed in place and cannot move.
