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chem chapter 1
grade 11 chem chapter 1
| Question | Answer |
|---|---|
| who created the basic idea of atoms and their behaviour? | Dalton |
| what was used to discover the electron? | cathode ray tube |
| who discovered the electron? | thomson |
| what is the raison bun model? | the theory that thomson had on the model of the atom. The atom was a "bun" and the "raisons" were electrons embedded in it |
| what experiment did rutherford conduct? what results did he discover? | he aimed tiny positive alpha particles at a thin sheet of gold foil. Although most went through the foil, some deflected and some bounced back |
| what did rutherford discover? | the nucleus and protons |
| what was rutherford's ideas about the atom? | they were mostly empty space and electrons take up very little space and very little mass |
| who discovered neutrons? | james chadwick |
| what happens to electron to determine the wavelength (colour) of light? | electrons are jumping to and from energy levels |
| what is an isotope? | when there are two or more forms of the same element. elements with the same atomic number but different numbers of neutrons which will result in different atomic masses. |
| what is the octet rule? | generally when ions combine, they tend to achieve 8 valence electrons and become stable |
| rubbing different materials together can make them acquire what? | static electricity |
| what are the compounds called with oppositely charged ions that are grouped close together and form crystals? | ionic solids |
| what does multivalent mean? | property of having more than one possible valence |
| what is a polyatomic ion? | an ion made up of more than one atom that acts as a single entity |
| what 6 elements are most present in the body in order of abundance by mass? | oxygen, carbon, hydrogen, nitrogen, calcium and phosphorus |
| do metals become anions or cations? | they tend to lose their electrons becoming cations (positive charge) |
| do non metals become anions or cations? | they tend to gain electron becoming anions (negatively charged) |
| are polyatomic ions usually anions or cations? | almost all are anions |
| how do ions exists in the body? | they are dissolved in water |
| what does a group indicate? | the number of valence electrons |
| what does a period indicate? | the number of energy levels |
| what group is so reactive that they can only exist as compounds? | alkali metals |
| what happens to alkali metals when exposed to air? | they turn white because they form oxides |
| what charge does alkaline earth metals possess? | they lose 2 to become a cation with a charge of +2 |
| what group occurs in all 3 states? | halogens |
| what are 3 characteristics of noble gases? | all gases, non reactive, stable |
| what is the name of the complex metals that are multivalent? | transition metals |
| define periodic law | when the elements are arranged in order of increasing atomic number, their properties show a periodic recurrence and gradual change |
| define effective nuclear charge | the attraction between an electron of an atom and the nucleus |
| define shielding effect | electrons from the inner energy levels shield outer electrons from the nucleus |
| what happens to the atomic radius when moving down a group? why? | radius increases. added energy levels make valence electrons further from the nucleus |
| what happens to the atomic radius when moving across a period? why? | radius decreases. protons are added but energy levels are not, so nuclear charge increases, pulling electrons closer to nucleus |
| does losing an electron make an atom bigger or smaller? why? | makes it smaller. repulsion is weaker. more protons than electrons, electrons are drawn towards nucleus |
| does gaining an electron make an atom bigger or smaller? why? | makes it bigger. repulsion is stronger. more electrons than protons and electrons are not drawn towards nucleus |
| what is ionization energy? | amount of energy needed to remove an electron |
| moving down a group, does ionization energy increase or decrease? why? | decreases because less energy is needed to remove an electron since the radius is bigger and nuclear charge is weaker |
| moving across a period, does ionization energy increase or decrease? why? | increases because more energy is needed to remove an electron since the radius is bigger and nuclear charge is stronger |
| what is electron affinity? | the energy change when an atom gains an electron |
| moving down a group, does electron affinity increase or decrease? why? | decreases because less energy is gained when electrons are farther from the nucleus since nuclear charge is weaker |
| moving across a period, does electron affinity increase or decrease? why? | increases because more energy is gained when electrons are closer to the nucleus since nuclear charge is stronger |
| what has stronger IE and EA, metals or non metals? | non metals |
| what is electroegativity? | the tendency of an atom to pull electrons towards itself |
| moving down a group, does electronegativity increase or decrease? | decreases |
| moving across a period, does electronegativity increase or decrease? | increases |
| what is the most electronegative element? | fluorine |
| what is the least electronegative element? | Cs and Fr |
| when do metals increase in reactivity? why? | moving down and left, because they have a weaker hold on their valence electrons |
| when do non metals increase in reactivity? why? | moving up and right because they have a higher electron affinity when they are smaller |
Created by:
caitlyn.kummer
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