Atoms, Ions, and Reactions
No description yet. This curated deck is ready for daily study.
Card preview (24)
Lab rules
• Avoid skin and eye contact with all chemicals • Do not mess around • Avoid distracting or startling people • Use equipment only for its designated purpose. • Do not taste or intentionally sniff chemicals. • Wash hands prior to leaving the laboratory. • Long hair and loose clothing must be pulled back • Laboratory safety glasses or goggles should be worn • Closed toe shoes will be worn at all times
To describe the specialist science areas
Physics: Properties of matter and energy Biology: Living organisms Chemistry: Substances of which matter is composed Astronomy: The study to explain everything we observe in the universe
To identify and state the functions of common lab equipment
To correctly draw scientific equipment
Describe the structure of the atom
(2,8,8) Charge | Mass | Location Proton | +1 | 1 | nucleus Neutron| 0 | 1 | nucleus Electron| -1 | 0 | orbitals, shells
Describe the key differences between the three subatomic particles
Proton: positive charge Electron: negative charge, the lightest mass Neutron: neutral charge
Determine the structure of the atom (number of p, n, e-) based on data from the periodic table
Draw the arrangement of electrons around any given atom
Define an ion
Any atom or group of atoms that bears one or more positive or negative electrical charges.
Describe the role of electrons in chemical reactions
Metal elements lose electrons to form posive ions (cations) and non-metal elements gain electrons to form negave ions (anions) when they react.
Explain why elements form ions of a specific charge (link to number of valence electrons)
They want to form a full valence shell and want a noble gas configuration, as this stabilises the element and therefore makes it less reactive.
Describe and determine the structure of simple mono-atomic ions (number of p, n, e-) based on data from the periodic table
Draw the electron arrangement around any given mono-atomic ion
Determine the number of atoms of each element / total number of atoms in a compound, given its chemical formula
examples: H20 = 2 elements but 3 atoms PCl5 = 2 elements but 6 atoms HCl = 2 elements but 2 atoms Cl2 = 1 element but 2 atoms
State the chemical name of an ionic compound from a given formula
Ion state of oxygen becomes oxide, e.g same for ammonium, carbonate, hydrogen carbonate, sulfate, nitrate, hydroxide
Explain why elements combine in exact ratios to make electrically neutral compounds (ionic bonding)
Positively charged atoms are attracted to negatively charged atoms because they want to form a neutral compound. Example: Mg2+ and Cl- to become neutral there needs to be 2 positive and 2 negatives (because Mg has a positive charge of 2 already). Therefore, the answer is = MgCl2.
Apply information from the table of ions to construct ionic formulae
Some compounds are still reactive (have a charge) after they have reacted together, making it a NOT neutral compound. This is known as the table of ions. Example: Calcium carbonate. Carbonate is a NON neutral compound = CO(lower 3)(charge 2-). Calcium = Ca2+.
Define the terms ‘reactants’ and ‘products’
Reactants: The substances that are reacting together are called reactants. Products: The substances or substances produced are called products.
Why is matter conserved during chemical reactions
Matter is conserved during chemical reactions because in an equation there cannot be a product of something when there wasn’t a reaction (vice versa).
Write word equations for chemical reactions
Tip: All group 17 are diatomic atoms as well as oxygen and hydrogen.
Explain the point of balancing a chemical equation
Chemical equations are balanced so that there is no extra atoms left on the reactant or product side.
Apply knowledge of chemical formulae to balance simple equations limited to formation of one product (not acid reactions)
Describe and explain covalent bonds
When two or more atoms have a shared pair of electrons. They do this so it can be more stable and the bond is very strong.
Explain molecules
Two or more atoms covalently bonded together.