Atomic Structure and Periodic Table HL quizzes
Quiz 1 Ionic Bonding 1. Atoms will bond to attain a f o s of e (2 marks) 2. When metal atoms bond they always electrons to form ions ( ions). 3. When non-metal atoms react with metals, they always electrons to form ions ( ions). 4. Sodium is in group 1 which means it will lose negative electron and become an Na ion. 5. Magnesium is in group 2 which means it will lose negative electrons and become an Mg ion. 6. Aluminium is in group 3 which means it will lose negative electrons and become an Al ion. 7. When bonding to a metal Chlorine (group 7) will gain negative electron and become a Cl ion. 8. When bonding to a metal Oxygen (group 6) will gain negative electrons and become an O ion. 9. Positive and negative ions hold together because charges attract.
Quiz 2 ionic structures and properties 1. Ionic compounds have melting and boiling points. 2. Ionic compounds can only conduct electricity when they are or, this is because the ions become free to and carry. (4 marks) 3. Ionic compounds are all quite easy to in water. 4. Draw a diagram of the structure of an ionic solid (you only need to draw 9 ions, please label the charges) (2 marks) 5. Ionic structures are large and regularly arranged so we call them a G Ionic L 6. The forces of attraction between the positive and negative ions are called forces of attraction.
7. Draw a diagram to show the covalent bonding in carbon dioxide (outer shell only 7 electrons each). (2 marks) Quiz 3 Covalent bonding 1. Covalent bonding only involves - atoms. 2. In covalent bonding electrons are between atoms. 3. One electron can be shared by each atom involved, these are called s bonds, if two electrons are shared by each atom involved these are called d bonds. (2 marks) 4. Small structures made of more than one atom that are covalently bonded together are called 5. Many gases are covalent substances for example air contains and that are covalent substances. 6. Draw a diagram to show the covalent bonding between two chlorine atoms (outer shell only 7 electrons each). (2 marks)
Quiz 4 Covalent molecules and properties 1. Small covalent molecules are called s 2. The atoms in these molecules are joined by strong covalent bonds, but the molecules are only held together by - forces. (2 marks) 3. This means that the molecules have low/high melting and boiling points. 4. This makes these substances normally or at room temperatures. 5. Compounds made of simple molecules do not conduct electricity because they do not have that are free to move. 6. Polymers are long molecules held together by bonds. 7. The intermolecular forces between polymer molecules are relatively so polymers are at room temperature. (2 marks)
Quiz 5 Properties of Polymers and Giant Covalent structures 1. Polymers are long chains this means that their inter-molecular forces are stronger/weaker than smaller molecules. 2. Draw two diagrams one to show the structure of the carbon molecules in diamond, one to show the structure of the carbon molecules in graphite. (2 marks) Diamond: Graphite: 3. In diamond each carbon atom has (number) strong covalent bonds to other carbon atoms. 4. In graphite each carbon atom has (number) strong covalent bonds to other carbon atoms, the last electron becomes.(2 marks) 5. A single layer of graphite is called. 6. What is the scientific name of silica? 7. Draw a diagram of silica.
Quiz 6 Properties of Diamond and Graphite 1.Diamond is the naturally occurring substance on the Earth. 2.Diamond and graphite both have high/low melting and boiling points because of their strong bonds. (2 marks) 3. doesn t conduct electricity but does because it has delocalised electrons that move and carry. (2 marks) 4. can be used as a lubricant because it has that off, due to the weak inter-molecular forces between them. (2 marks) 5.Graphene (a single layer pf graphite) is extremely strong but also very, making it useful for adding strength to materials. 6.Spheres or tubes of carbon atoms are generally called f. These structures can be used to cage other chemicals such as
Quiz 7 Metallic Bonding, changes of state. 1. Metals are formed only from ions, with the electrons they have lost spread between the ions. 2. These electrons are d, and able to move which means metals can and heat. (2 marks) 3. Metals have a regular structure (that we call a l ) and this also means they have that can slide over each other, meaning we can shape metals (they are m.) (2 marks) 4. Alloys are harder than pure metals because their have been disrupted by having different sized. 5. Draw a diagram that shows the three different states, on the arrows between them label the four different state changes (s to l, l to g, g to l, l to s). (2 marks) 6. What is required for a substance to move towards a gas? 7. What is the temperature at which an object freezes called?