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SCience test
| Chemistry | the study of matter |
| Matter | anything that takes up space and has Mass |
| Non-matter | energy, feelings, time |
| Atoms | the building blocks of matter. what everything is made of. |
| Atoms sub-atomic particles | protons, neutrons and electrons |
| Types of atoms | there are 118 types of known atoms |
| Columns | Groups |
| Rows | Periods |
| Atomic Number | How and atom is identified by the number of protons |
| Stable atoms | Number of electrons is the same to the number of protons |
| Relative Atomic Mass | Mass of an atom, made up of protons added to neutrons |
| Number of Valence electrons | Depends on group. Noble Gases have full valence shells. |
| Number of Valence shells | Depends on period. |
| Cation | Metal ion loses or donates electrons have a positive charge due to there being more protons then electrons Group 1 + 2 loses electrons (ignore hydrogen) |
| Ions | an atom that loses or gains electrons to produce an overall charge and gain a full valence shell done through chemical reactions balanced, unstable |
| Anion | Non-Metals shares or gains electrons have a negative charge due to there being less protons then electrons |
| Electronic Configuration | 2, 8, 8, 2 |
| Reactivity of metals | Group 1 Period 2-7 Alkali Metals lose 1 electron = most reactive Group 2 Period 2-7 loses 2 electrons = less reactive Group 1 is always most reactive Greater period = greater reactive Less electrons missing = more reactive |
| Metallic Bonding | M+M Forms Lattice Structure M atoms bond by sharing electrons Valence electrons become delocalised, moves freely held together by the force of attraction between cations and electrons |
| Metal ion: Lithium | P= 3 E = 3 N = 4 loses 1 electron P= 3 E = 2 N = 4 Charge is 1+ or + |
| EXCEPTION to Non-Metals | Group 18 = full valence shell =/= ions Hydrogen = cation Carbon = cation |
| Reactivity of non-metals | Group 18 = Noble Gases Group 17 = Halogens Group 1 is always most reactive Greater period = less reactive Valence shells are close to nucleus = strong attraction to electrons |
| Properties of Metals | Conductors: can conduct heat and electricity Malleable: Can be hammered into different forms like sheet Ductile: can be drawn into a wire Solid at room temperature: Applies to but mercury who it built different <3 shiny |
| Properties of Non-metals | Liquids, gases, metalloid range of colours not shiny Metalloid can be semi-conductors (only conduct electricity) No free moving electrons, held within valence shell Weak force between molecule making them have low melting/boiling point |
| Covalent Bonding | NM+NM Merges valence shells balance atom do this to merge valence shells to share electrons Examples H^2, O^2, NH^3 |
| Ionic Bonding | M + NM When an atom which needs to lose one electron donates it to another atom that needs to gain electrons creates a pair of ion that are attracted to each other lattice structure |
| Chemical Formula | The short hand way of representing which ions are present on the ionic structure and the ratio of these ions in the lattice. |
| STEPS TO WRITING CHEMICAL FORMULA | 1. identify relevant ions in formula sheet, write down symbol and charge 2. check if charges balance (are they the same) 3. if charges do not balance, add an ion one at a time 'til they do To be continued |
Created by:
St4dent
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