Atoms, Ions, and Reactions

Question 1

Lab rules

Answer 1

• 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

Question 2

To describe the specialist science areas

Answer 2

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

Question 3

To identify and state the functions of common lab equipment

Question 4

To correctly draw scientific equipment

Question 5

Describe the structure of the atom

Answer 5

(2,8,8)
Charge | Mass | Location
Proton | +1 | 1 | nucleus
Neutron| 0 | 1 | nucleus
Electron| -1 | 0 | orbitals, shells

Question 6

Describe the key differences between the three subatomic particles

Answer 6

Proton: positive charge

Electron: negative charge, the lightest mass

Neutron: neutral charge

Question 7

Determine the structure of the atom (number of p, n, e-) based on data from the periodic table

Question 8

Draw the arrangement of electrons around any given atom

Question 9

Define an ion

Answer 9

Any atom or group of atoms that bears one or more positive or negative electrical charges.

Question 10

Describe the role of electrons in chemical reactions

Answer 10

Metal elements lose electrons to form posive ions (cations) and non-metal elements gain electrons to form negave ions (anions) when they react.

Question 11

Explain why elements form ions of a specific charge (link to number of valence electrons)

Answer 11

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.

Question 12

Describe and determine the structure of simple mono-atomic ions (number of p, n, e-) based on data from the periodic table

Question 13

Draw the electron arrangement around any given mono-atomic ion

Question 14

Determine the number of atoms of each element / total number of atoms in a compound, given its chemical formula

Answer 14

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

Question 15

State the chemical name of an ionic compound from a given formula

Answer 15

Ion state of oxygen becomes oxide, e.g same for ammonium, carbonate, hydrogen carbonate, sulfate, nitrate, hydroxide

Question 16

Explain why elements combine in exact ratios to make electrically neutral compounds (ionic bonding)

Answer 16

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.

Question 17

Apply information from the table of ions to construct ionic formulae

Answer 17

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+.

Question 18

Define the terms ‘reactants’ and ‘products’

Answer 18

Reactants: The substances that are reacting together are called reactants.

Products: The substances or substances produced are called products.

Question 19

Why is matter conserved during chemical reactions

Answer 19

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).

Question 20

Write word equations for chemical reactions

Answer 20

Tip: All group 17 are diatomic atoms as well as oxygen and hydrogen.

Question 21

Explain the point of balancing a chemical equation

Answer 21

Chemical equations are balanced so that there is no extra atoms left on the reactant or product side.

Question 22

Apply knowledge of chemical formulae to balance simple equations limited to formation of one product (not acid reactions)

Question 23

Describe and explain covalent bonds

Answer 23

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.

Question 24

Explain molecules

Answer 24

Two or more atoms covalently bonded together.

Question 25

Explain diatomic atoms

Answer 25

Diatomics are always molecules as they are (only) two atoms covalently bonded together.

Question 26

What is an atom

Answer 26

An atom is thought to be the building blocks of matter

Question 27

What is an element

Answer 27

A structure made up of one type of atom

Question 28

Who ‘created’ the periodic table

Answer 28

Dimitri Mendeleev, he arranged them based on how heavy they were and found a pattern.

Question 29

What is an mono-atomic atom

Answer 29

Mono-atomic means there is one atom of an element. To have a positive charge you loose electrons and to have a negative charge you gain electrons.