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Chemistry
Periodic table and atomic structure - Unit 3
| Question | Answer |
|---|---|
| What are group 1 elements also known as? | Alkali metals |
| What are group 2 elements also known as? | Alkaline earth metals |
| What is the d-block also known as? | Tranisiton metals |
| What are group 7 also known as? | Halogens |
| What are group 8/0 also known as? | Noble gases |
| Where do metals lie? | To the left of the striarcase |
| Where do non-metals lie? | To the right of the staircase |
| What is the mass number? | Sum of number of protons and neutrons |
| What is atomic number? | The number of electrons |
| What is an isotope? | An atom with the same number of protons and electrons but differant numbers of neutrons |
| What must be used to veiw an emissions spectra? | Spectroscope |
| How can energy be provided to a solid sample? | Flame testing |
| How can energy be provided to a gaseous sample? | Electrical discharge tube at low pressure |
| What causes the release of light giving the emission spectra? | Electrons falling back to their normal quantum shell, having jumped up energy levels |
| What is ionization energy? | Energy required to remove one mole of gaseous electrons from one mole of gaseous atoms |
| Which element gives a lilac flame? | Pottassuim |
| Which elelment gives a Yellow flame? | Soduim |
| Which two elements give a red flame? | Lithium and strontuim |
| Which element gives a brick red flame? | Calcuim |
| Which element gives no flame colour? | Magnesuim |
| Which element gives an apple green flame? | Barium |
| Which element gives a blue/green flame? | Copper |
| Which quantum levels are easier to remove electrons from? | Outer |
| What does a jump in ionization energies indicate? | A change of quantum level |
| What happens to ionization energies as you move across the period? | They increase |
| What happens to ionization energies as you move down the group? | They decrease |
| How are electrons arranged? | In quantum shells |
| What are the 3 first subshells? | s,p,d |
| How many electrons fit into the s sub-shell? | 2 |
| How many electrons fit into p sub-shell? | 6 |
| How many electrons are found in sub-shell d? | 10 |
| In what order are the sub-shells illed? | s, p, d |
| What causes chemical simularities down the groups? | Simular electron arrangements |
| What is electron affinity? | Energy change occuring when one mole of gaseous electrons are added to one mole of gaseous atoms |
| What are the two types of compounds? | Giant and molecular |
| What are the 3 types of chemical bonding? | Metallic, covalent, ionic |
| What type of bonding is found in molecular compounds? | Covalent |
| What type of bond in found in giant compounds? | Metallic, covalent, ionic |
| What size are positive ions in relation to their elements? | Smaller |
| What size are negative ions in relation to their elements? | Larger |
| What keeps the crystalline shape? | Attraction from differant ions, repulsion from same ions |
| What are high melting points of metals caused by? | Metallic bonding |
| What is high thermal conductivity of metals caused by? | Metallic bonding |
| What is high electrical conductivity of metals caused by? | Metallic bonding |
| What is the model for metallic bonding? | Metal ion surronded by electrons |
| Does metallic bonding acount for all metal properties? | No |
Created by:
1988kayla
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