Chemistry

Question 1

Define Matter.

Answer 1

Matter is any substance that has mass and takes up space.

Question 2

All matter is made up of…?

Answer 2

Atoms.

Question 3

Describe subatomic particle placement within the atom.

Answer 3

Protons and neutrons located within the nucleus, with electrons in orbitals surrounding the nucleus.

Question 4

Recall the charge and mass of protons, neutrons and electrons.

Answer 4

Proton—positive 1
electron—negative negligable
neutron—no charge 1

Question 5

What does the atomic number and mass number represent?

Answer 5

Atomic number is how many protons an element has. Mass number is the number of protons and neutrons.

Question 6

How can subatomic information be used to identify an element?

Answer 6

The number of protons in the nucleus determines which element an atom is.

Question 7

Recall the number of electrons in electron shells.

Answer 7

The innermost shell has a maximum of two electrons but the next two electron shells can each have a maximum of eight electrons.

Question 8

How are elements ordered in the periodic table?

Answer 8

The chemical elements are arranged in order of increasing atomic number （number of protons).

Question 9

Recall the difference between physical and chemical properties.

Answer 9

Chemical properties can only be observed or measured when a substance undergoes a chemical change. Physical properties are properties that can be observed without a chemical change.

Question 10

Recall physical and chemical properties of metals.

Answer 10

Shiny
High Melting Point
Good conductor of electricity and heat
Not brittle

Question 11

Recall physical and chemical properties non-metals.

Answer 11

Low melting point
Dull appearance
Low density
Poor conductor

Question 12

Elements in the same group have similar properties as they have…?

Answer 12

The same number of valance electrons, and electron configuration.

Question 13

How does electron configuration of an atom determine its position on the periodic table?

Answer 13

The number of valance electrons determines the group the element resides in. The number of electron shells it has determines it’s period.

Question 14

Describe the difference between an atom and an ion.

Answer 14

Atoms are neutral, whereas ions have a charge.

Question 15

Describe the difference between an anion and a cation.

Answer 15

An anion is a negatively charged ion. A cation is a positively charged ion.

Question 16

Explain why some metals are more reactive than others.

Answer 16

Metals with a greater total number of electrons tend to be more reactive as their outermost electrons (the ones which will be lost) exist further from the positive nucleus and therefore they are held less strongly by electrostatic attraction.

Question 17

Define monoatomic.

Answer 17

A molecule composed of just one atom, and lacking any covalent bonds

Question 18

Define polyatomic.

Answer 18

A molecule containing two or more two atoms.

Question 19

What makes a compound metallic?

Answer 19

A metallic compound is formed when there exists a bond between two metals or one metal with another non-metal/an ionic group

Question 20

What makes a compound ionic?

Answer 20

Ionic bonding occurs through a process called electron transfer, where one atom gives electrons to anotherThe elements in the compound are metal and non-metal, then the bonding will be ionic

Question 21

What makes a compound covalent?

Answer 21

A covalent compound is made when two or more nonmetal atoms bond by sharing valence electrons

Question 22

Ionic compounds involve a … of valance electrons for … ?

Answer 22

Transfer
Stability

Question 23

Covalent compounds involve a … of valance electrons for …?

Answer 23

Sharing
Stability

Question 24

Describe the difference between monoatomic and polyatomic compounds.

Answer 24

Monatomic ion is formed when an electron is lost or gained from a valence shell whereas polyatomic ions are formed between atoms that are held together by forces of attraction.

Question 25

How do ionic compounds form between a metal and a non-metal.

Answer 25

The metal loses electrons and becomes positively charged and the non-metal gains electrons and becomes negatively charged.

Question 26

What holds together ions in an ionic compound?

Answer 26

Electrostatic attraction.

Question 27

The strength of electrostatic attraction determines..?

Answer 27

The properties of the compound.

Question 28

Compounds with the suffice ide are …?

Answer 28

monoatomic ions

Question 29

Compounds with the suffice ate are …?

Answer 29

Polyatomic

Question 30

How to use the ionic formula to predict the charge on a transition metal?

Answer 30

Drop and swap with its partnering ion

Question 31

Use collision theory to describe how a chemical reaction takes place.

Answer 31

Collision theory states that the reacting particles must collide with one another.

Question 32

Products are…?

Answer 32

On the right side of a chemical equation.

Question 33

Reactants are…?

Answer 33

On the left side of the chemical equation.

Question 34

How does the law of conservation of mass explain why chemical equations must be balanced?

Answer 34

According to this law the mass of products must be equal to the mass of reactants.

Question 35

Classify and predict the products for a combustion reaction.

Answer 35

Complete.
Products will always be carbon dioxide (CO2) and water (H2O)

Question 36

Classify and predict the products for a double replacement reaction.

Answer 36

Precipitation and nuetralisation reactions
Change the partners of the anions and cations on the reactant side to form new compounds.
AB+CD→ AD+CB

Question 37

Classify and predict the products for a combination reaction.

Answer 37

Synthesis
The product will be a simple compound containing both elements.
A+B→ AB

Question 38

Classify and predict the products for a decomposition reaction.

Answer 38

A decomposition reaction occurs when one reactant breaks down into two or more products.
AB → A + B

Question 39

Define reaction rate.

Answer 39

The rate of reaction is the speed at which a chemical reaction takes place.

Question 40

Describe the relationship between frequency of collisions and reaction rate.

Answer 40

Collision theory states that the rate of a chemical reaction is proportional to the number of collisions between reactant molecules. Therefore more/less collision result in faster/slower reaction rate.

Question 41

Describe how temperature, surface area and a catalyst affect reaction rate.

Answer 41

Increasing temperature increases the rate of a chemical reaction. A larger surface area of reactants leads to an increase in the reaction rate. A catalyst is a substance that increases the rate of a chemical reaction by providing an alternative reaction pathway with lower activation energy. All speed/slow the rate of reaction depending on whether its increased/decreased.

Question 42

Explain how a catalyst increases reaction rate, but is not used up in a chemical reaction.

Answer 42

A catalyst works by providing an alternative reaction pathway that has a lower activation energy compared to the pathway without the catalyst. After the reaction, the products are desorbed from the catalyst’s surface, leaving the catalyst unchanged.