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chemistry > atomic structure and periodic table > Flashcards

atomic structure and periodic table Flashcards

1
Q

what do atoms have a radius of

A

about 0.1 nanometer (that’s 1x10^-10 metres

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2
Q

describe the structure of an atom use the terms proton, neutron, electron, nucleus and shell in answer

A

atoms have a small nucleus surrounded by electrons. The nucleus is in the middle of the atom and contains protons and neutrons. The electrons occupy shells around the nucleus

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3
Q

what is the relative size of the nucleus compared to the atom

A

the nucleus is about 1/10,000 the size of an atom

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4
Q

whats the relative charge of :
proton
neutron
electron

A

proton: +1
neutron: 0
electron: -1

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5
Q

what is the relative mass of a proton

A

1

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6
Q

are atoms uncharged particles?. Explain why

A

Theyre uncharged particles as they have the same number of protons as electrons and protons and electrons have opposite chargers of the same size, so cancel each other out

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7
Q

how does an atom become an ion

A

if some electrons are added or removed the atoms become charged and is then an ion

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8
Q

what decides what type of atom it is

A

its the number or protons in the nucleus that decides what type of atom it is

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9
Q

an atom w one proton in its nucleus is hydrogen

A
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10
Q

an atom w two protons is helium

A
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11
Q

whats an ion?

A

its an atom or group of atoms that has lost or gained electrons

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12
Q

definition of acid

A

a substance that releases h+ ions in water (pH<7)

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13
Q

give examples of bases

A

sodium hydroxide - NaOH, potassium hydroxide - KOH, calcium hydroxide - Ca(OH)2, ammonia - NH3

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14
Q

definition of base

A

a substance that reacts with an acid to form a salt

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15
Q

whats a alkali

A

a soluble base (pH>7)

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16
Q

whats an indicator

A

a chemical that changes colour depending on whether it’s an acid or alkali

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17
Q

what does metal oxide + acid go to
e.g. copper oxide + sulfuric acid –> ….

A

metal oxide + acid —> salt + water
copper oxide + sulfuric acid –> copper sulfate + water

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18
Q

why will reacting a metal oxide with an acid not produce an alkali solution

A

when reacting a metal oxide with an acid, it will not produce an alkali solution due to the excessive metal oxide not reacting

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19
Q

metal + acid –> ….
magnesium + sulfuric acid –>

A

metal + acid –> salt + hydrogen (MASH)
magnesium + sulfuric acid –> magnesium sulfate + hydrogen

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20
Q

metal carbonate + acid –>
magnesium carbonate + sulfuric acid–>

A

metal carbonate + acid –> salt + water + carbon dioxide
magnesium carbonate + sulfuric acid –> magnesium sulfate + water + carbon dioxide

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21
Q

metal hydroxide + acid –>
sodium hydroxide + hydrochloric acid –> …

A

metal hydroxide + acid –> salt + water
sodium hydroxide + hydrochloric acid –> sodium chloride + water

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21
Q

how was Mendeleev’s periodic table arranged

A

arranged in order of atomic weight - however some elements were swapped over to fit with the properties of other elements in the group
left gaps

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21
Q

why did Mendeleev leave gaps in periodic table

A

Mendeleev predicted properties of undiscovered elements and when they were discovered, his predictions were correct

22
Q

why weresome scientists skeptical about Mendeleevs table

A

because he mixed metals and non metals and some boxes contained two elements

23
Q

what ions did metals have

A

positive ions

24
Q

what ions do non metals have

A

negative ions

25
Q

how is the modern periodic table arranged

A

ordered in increasing atomic number

26
Q

why do things in the same group react in a similar way

A

they have the same number of outer shell electrons

27
Q

periodicity definition

A

a repeating pattern of properties at regular intervals

28
Q

tip - metallic bonding

why do metals have a high melting point

A

a lot of energy is needed to overcome the strong electrostatic force of attraction between metal ions and delocalised electrons

29
Q

why r metals a good electrical conductor

A

delocalised electrons can move and carry charge

30
Q

why r metals malleable/ductile

A

positive metal ions are arranged in neat rows that can slide past each other whilst remaining bonded

31
Q

tip - covalent bonding

why do non metals have low melting points

A

not a lot of energy is needed to overcome weak intermolecular forces between molecules

32
Q

tip - covalent bonding

why r non metals electrical insulators

A

molecules have no overall charge - no charged particles are free to move

33
Q

why might noble gases be used for filling lightbulbs

A

they have no need to gain or lose electrons as they have full outer shells of electrons this means they r inert

34
Q

what do noble gases exist as

A

monatomic gases .they exist as gases at room temp due to weak forces between atoms

35
Q

why does boiling point increase down the group (0/noble gas)

A

increases due to atoms increasing in size (increasing atomic number) so forces r stronger so more energy is needed

36
Q

alkali solution is due to prescence of what

A

alkali solution is due to the prescense of hydroxide (*OH-) ions

37
Q

metal + water –>

A

metal + water –> metal hydroxide + hydrogen

38
Q

metal + chlorine –>
e.g. 2Na + Cl2 –>

A

metal + chlorine –> metal chloride
2NaCl

39
Q

Metal + oxygen –>
e.g. 4K + O2 –>

A

metal + oxygen –> metal oxide
4K + O2 –> 2K2O

40
Q

As group 1 (alkali metals) increase in atomic number (down group) what happens to :
density
strength
melting point
reactivity

A

density increases
strength increases
melting point decreases
reactivity increases

41
Q

what does reactivity depend on

A

depends on how easily the outer electrons is lost to form a 1+ ion

42
Q

why does reactivity increase down group 1 (alkali metals)

A

increased atomic radius - outer electron is further from nucleus
increased electron shielding - more full electrons shells between the outer electron and nucleus
decreased nuclear attraction to outer electron so it is more easily lost

43
Q

what do group 7 (halogens) exist as

A

diatomic molecules when each atom shares 1 electron in the covalent bond

44
Q

down group 7 (halogens) why does melting + boiling point increase

A

as the molecules increase in mass the intermolecular forces increase in strength so more energy is needed to overcome them

45
Q

what do halogens react w metals to form and what bonding does it have

A

to form halide ions (F-,BR- ect) by gaining an electron the product has ionic bonding

46
Q

when halogens react w non metals what molecules does it form e.g. H2 +Cl2 –>

A

form covalent molecules e.g. H2 + Cl2 -> 2HCl

47
Q

what does the more reactive halogen displace

A

more reactive halogen displaces the less reactive of halogen from a compound

48
Q

order of these most reactive - least reactive
iodine,chlorine.astatine.bromine

A

most reactive
chlorine
bromine
iodine
least reactive
astatine

49
Q

what would happen to this equation if displacement happened:
KBr + Cl2 –>

A

KBr + Cl2 –> 2KCl + Br2

50
Q

when halogens react what do they gain

A

when halogens react they gain an electron

51
Q

why does reactivity decrease down group 7 (halogens)

A

atomic radius increases - electron gained is further away from nucles
electron shield increases - more full electron shells between nucleus and electron to be gained
weaker force of attraction between nucleus and electron to be gained so therefore gaining of electron is harder

52
Q

what r properties of transition metals (list 5)

A

high melting point,high density, high strength, high hardness, low reactivity

53
Q

why is iron used for construction

A

hard and strong + low reactivity

54
Q

definition of catalysts

A

substance that speeds up rate of a reaction without being used up

chemistry (4 decks)

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