Mid Topic Test Term 1 (Chemistry) Flashcards
Proton (Charge)
Positive
Proton (Location)
Nucleus
Proton (Relative Size)
x 1836
Electron (Charge)
Negative
Electron (Location)
Electron Shells
Electron (Relative Size)
x1
Neutron (Charge)
0
Neutron (Relative Size)
x 1836
Neutron (Location)
Nucleus
Atomic Number
The number of protons and electrons in the atom.
Atomic Mass
The average number of protons and neutrons in the atom.
Element
A pure substance consisting only of one type of atom that all have the same numbers of protons in their nucleus. (Cannot be broken down into simpler substances).
Compound
A chemical substance is composed of many identical molecules composed of atoms from more than one element held together by chemical bonds.
Transition Metals
Properties:
- High melting and boiling points
- Solid at room temp
- Physical properties like metals
- Chemical properties like non-metals
Halogens
Properties:
- Highly Reactive
- Low Melting and Boiling Points
- Reactivity decreases down the table group.
- Exist as diatomic molecules.
Noble Gases
Properties:
- Unreactive non-metal gases
- Low density
- Non-flammable
- Low boiling points
- Bp and density increase down the group
Alkali Metals
Properties:
- Low melting and boiling points
- Very soft
- React with water to produce a metal OH- solution and hydrogen gas
- Reactivity increases down the group
- All are highly reactive
Alkaline Earth Metals
- All shiny
- Low melting and boiling points
- Reactivity increases down the group.
- React with halogens to form ionic salts.
- All apart from beryllium react with water to form OH-.
Alkali Metals trend
Increases reactivity down the group.
Alkaline Earth Metals trend
Increases reactivity down the group.
Halogens trend
Decreases reactivity down the group.
Metal Location on periodic table
Everything apart from the edge of Boron.
Non-metal location on periodic table
Edge of Boron to the rest of the right side.
Boron
Group 13 Period 2
Iodine
Group 17 Period 5
Calcium
Group 2 Period 4
Beryllium
Group 2 Period 2
Maximum Electron Configuration
2 8 8 2
Valence Electron
Electrons in the outermost shell of the atom that determine an atom’s or group’s ability to bond with others.
Ionic Bond
A type of chemical bonding that involves the attraction between oppositely charged ions with sharply different electronegativities.
Ionic Bond Formation
Formed when atoms gain or lose e-. Formed when electrons are transferred between atoms.
Covalent Bond
Involves sharing electrons because both elements have high electronegativities.
Covalent Bond formation
when the difference between the electronegativities of two atoms is too small for an electron transfer to occur to form ions, it rather shares electrons. The sharing can be equal (non-polar), or unequal (polar).
Metallic Bond
Arises from the electrostatic attractive force between conduction electrons and positively charged metal ions. It may be described as the sharing of free electrons among a structure of positively charged ions.
Metallic Bond Formation
Bonds between atoms in a metal held together by a crystalline lattice. (‘ In a sea of free electrons’).
The Octet Rule
Atoms are happy with a full valence shell.
Acheived by gaining or losing electrons.
Ion
any atom or group of atoms that bears one or more positive or negative electrical charges.
Cation
Positively charged ion
Cation Formation
When an atom loses one or more electrons: the loss of the negatively-charged electron(s) results in an overall positive charge.
Anion
Negatively charged ion
Anion Formation
Are formed from the gain of one or more electrons.
Polyatomic Ion
An ion with more than 1 type of atom. Usually a non-metal.
Group in periodic table
The vertical columns of the periodic table. Correspond to the number of valence shells.
Period in periodic table
The horizonal rows of the periodic table.
Correspond to the total number of shells.
What are the 3 types of chemical bonds
Metallic
Ionic
Covalent
What is a chemical bond?
What holds atoms together in molecules and enables the formation of chemical compounds.
Brittle
Hard but liable to break easily.
Malleable
Able to be hammered or pressed into shape without breaking or cracking.
Ductile
Ability to be drawn or plastically deformed without fracture.
Lustrous (Metallic Lustre)
The shiny appearance in metals.
