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Chem Notes #2
| Question | Answer |
|---|---|
| How many elements were identified by the year 1700? | 13 elements |
| Early chemists used the __________ of elements to sort them into groups. | |
| What is a triad? | a set of three elements with similar properties |
| How did Mendeleev arrange the elements in his periodic table? | in order of increasing atomic mass |
| The modern periodic table is arranged by ______ ______. | atomic number |
| Groups run ____, periods run ______. | down; across |
| What does each period correspond to? | a principal energy level |
| What is the periodic law? | when elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties |
| The further _____ you go across the periodic table, the less metallic the elements are. | right |
| Around __% of elements are metals. | 80 |
| Metals are generally ____ conductors of heat and electricity. | good |
| Most metals have ____ luster. | high |
| Are all metals solid at room temperature? | all except mercury(Hg) |
| What does ductile mean? | able to be drawn into a wire |
| What does malleable mean? | able to be hammered into thin sheets without breaking |
| Is there greater physical properties among metals or nonmetals? | nonmetals(solid, liquid, gas) |
| Nonmetals tend to have properties that are _________ to those of metals. | opposite |
| A metalloid generally has properties _______ to those of metals and nonmetals. | similar |
| Under different conditions, metalloids may act more similarly to a _____ or _________. | metal; nonmetal |
| What groups can elements be sorted into based on their electron configurations? | noble gases, representative elements, transition metals, or inner transition metals |
| 1a - 7a | representative elements |
| 1a | alkali metals |
| 2a | alkaline earth metals |
| 7a | halogens |
| 8a | noble gases |
| 1a-8a | # of valence electrons |
| What are the elements in Group B? | transition metals |
| Inner transition metals are the ___________ and _________, or the f. | lanthanides; actinides |
| The ________ between the nuclei of two identical atoms in a molecule can be used to estimate the ____ of atoms. | distance; size |
| How is the size of an atom expressed? | through atomic radius |
| How does atomic size generally change throughout the periodic table? | increases from top to bottom and decreases from left to right |
| Does an increase in positive charge draw electrons closer to the nucleus or push them away? | draws them closer |
| Does atomic radius increase as atomic number increases? | yes |
| What is an ion? | an atom or group of atoms with a charge |
| When do ions form? | when electrons are transferred between atoms |
| What is an ion with a positive charge called? | a cation |
| What is an ion with a negative charge called? | an anion |
| How are cations and anions formed? | cations are formed when atoms lose an electron and anions are formed when atoms gain an electron |
| Nonmetals tend to form _______, while metals tend to form ______. | cations; anions |
| What is ionization energy? | the energy required to remove an electron from an atom |
| First ionization energy is the energy required to remove the _____ electron from an atom. | first |
| Electrons can move to ______ energy levels when atoms absorb energy. Sometimes the electron has enough energy to ________ the attraction of the protons in the nucleus. | higher; overcome |
| How does first ionization energy tend to change across the periodic table? | decrease from top to bottom and increase from left to right |
| __________ ________ can help you predict what ions an element will form. | Ionization energies |
| The nuclear charge _________ across the period, but the shielding effect remains _______. | increases; constant |
| During reactions between metals and nonmetals, metals tend to ____ electrons and nonmetal atoms tend to ____ electrons. | lose; gain |
| Cations are always _______ than the atoms from which they form, while anions are always ______. | smaller; larger |
| Metals that are ______________ elements tend to lose all their outermost electrons during ionization. | representative |
| What is electronegativity? | the ability of an atom to attract electrons when the atom is in a compound |
| _________________ can be used to predict the type of bond that will form during a reaction. | Electronegativity |
| What is the most electronegative element? | fluorine |
| What is the least electronegative element? | cesium |
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alov9636
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