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32 Cards in this Set
- Front
- Back
Whatare the masses and charges of these parts of an atom? · Proton · Neutron · Electron |
Protons= +ve (mass1) Neutrons= neutral (mass1) Electrons= -ve (mass1/2000th) |
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Why do atoms usually haveno overall electrical charge? |
Atomsusually have no overall charge because they have equal numbers of protons (+ve)and electrons (-ve), which cancel one another out
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Allatoms of a particular element (e.g. carbon) all have the same number of what?
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Protons |
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Whatare the following numbers called? |
a= relative atomic mass b= atomic number
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Whatdo the numbers tell you about the atom? |
a= relative atomic mass – the number of protons and neutrons in the atom
b= atomic number – the number of protons (usually the same as the number ofelectrons) |
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Whatis an isotope?
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Anisotope is an atom with a different amount of neutronsY9
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Usethe periodic table to draw the electron structure of the following: -
· Neon · Calcium · Sodium Howcan you tell which group these atoms are in? |
Thenumber of electrons in the outer shell is the same as their group number
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Theelectron structure of sodium can be represented as 2,8,1 – what does this mean? Represent these atoms: -
· Fluorine · Oxygen · Potassium · Magnesium |
2,8,1means 2 electrons in the 1st shell, 8 electrons in the 2ndshell and 1 electron in the 3rd shell
Fluorine= 2,7 Oxygen= 2,6 Potassium= 2,8,8,1 Magnesium= 2,8,2 |
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How many electrons canoccupy the 1st and 2nd shell (energy level) of an atom?
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2in the 1st shell and 8 in the 2nd shell
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Whathappens to the electrons of 2 atoms when they chemically react?
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Duringa chemical reaction electrons are either given away, taken, or shared_ |
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Definethese terms: -
· Element · Compound · Mixture |
Element– a pure substance made from 1 type of atom only Compound– 2 or more elements chemically bound Mixture– 2 or more elements or compounds mixed together which are not chemically boundlass9^f |
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Whatis an ion? Howare +ve ions formed? Howare -ve ions formed?
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Anion is an atom with a charge +veions have lost electrons -veions have gained electrons |
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Explainhow the following atoms become ions (will they be +ve or –ve)?
· Potassium · Magnesium · Chlorine · Oxygen |
Potassium– loses 1 electron (K+) Magnesium– loses 2 electrons (Mg2+) Chlorine– gains 1 electron (Cl-) Oxygen– gains 2 electrons (O2-) |
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Use diagrams to show howthese atoms for ionic bonds: -
Sodium + Chlorine |
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Describeand use a diagram to show the structure of ionic compounds
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Ioniccompounds have a giant structure – they are bonded to 6 other ions byelectrostatic bonds
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Whatare the melting and boiling points of ionic compounds like? Whyis this? |
Ioniccompounds have high melting points and boiling points – to melt them you haveto supply enough energy to break the 6 bonds attached to each ion |
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Whathappens to the electrons when atoms form ionic bonds and covalent bonds? Whichis the strongest?
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Ionicbonds – 1 atom loses electrons and another gains electrons
Covalentbonds – electrons are shared Anindividual covalent bond is stronger than an ionic bond |
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Usediagrams to show how the following compounds are formed: -
· Hydrogen · Oxygen · Hydrogen Chloride |
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Usea diagram to show how water is formed
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Water(H2O)
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Howare the elements of the periodic table arranged?
Whatare the rows called? Whatare the columns called? |
Elementsare arranged in order of atomic number
Rowsare called periods Columnsare called groups |
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What are the melting andboiling points of covalent compounds like? Explain why this is
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Covalentcompounds have low melting and boiling points (are often gases) are there is noattraction between the molecules
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Whydo elements in the same group have similar properties?
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Elementsin the same group have similar properties as they all have the same number ofelectrons in their outer shell'>CE1
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Which2 elements would be out of order in the periodic table if they were arranged byatomic mass instead of atomic number?
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Potassiumand ArgonA
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Whatare the symbols for these compounds?
· Calcium carbonate · Sodium chloride · Hydrochloric acid |
Calciumcarbonate – CaCO3
Sodiumchloride – NaCl Hydrochloricacid - HCl |
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Why do covalent compoundsnot conduct electricity when dissolved?
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Covalentcompounds do not conduct because they do no break down into ions
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Givethe names of 3 covalent compounds which have giant ionic structures? Whatis the structure of each like?
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Diamond– 4 carbon-carbon covalent bonds Graphite– 3 carbon-carbon covalent bonds Silicondioxide – 2 double silicon-oxygen covalent bonds |
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Whydoes graphite conduct electricity?
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Graphiteconducts electricity because it is only bonded 3x (meaning there is adelocalised electron to pass the charge)
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Explainwhy ionic compounds have a giant structure
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Ioniccompounds have giant structures because the ions keep their charge and attractup to 6 other ions – forming a giant lattice
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Whatdoes monatomic mean and why are noble gases monatomic?
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Monatomic means an atom which only exists on its own (does not react) Noblegases are monatomic as they have a full shell and are un-reactive
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Whatdoes diatomic mean and why are elements such as the halogens, hydrogen andoxygen diatomic?
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Diatomic– atoms in pairs, e.g. H2 and O2
Halogenswill form diatomic molecules because they covalently bond with each other,forming pairs |
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What is the bonding inmetals like?
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The bonding in metalscreates delocalised electrons (free to move and pass on electrical current)
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Whydo metals conduct electricity?
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