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Sciene Chem > Atomic structure and periodic table 1 > Flashcards

Atomic structure and periodic table 1 Flashcards

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1
Q

What does the nucleus contain

A

protons and neutrons

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2
Q

What charge does the nucleus have

A

positive

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3
Q

what is the charge and mass of an electron

A

negatively charged and no mass

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4
Q

what is the charge and mass of a proton

A

positively charged and 1 mass

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5
Q

what is the charge and mass of a neutron

A

neutral charge and 1 mass

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6
Q

what happens to the equal charge when it is an ion

A

it changes depending on what is added to it

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7
Q

how do you calculate the number of neutrons

A

mass number - atomic number

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8
Q

what are isotopes

A

different forms of the same element which have the same amount of protons but a different amount of neutrons

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9
Q

what does the mass number contain

A

protons and neutrons

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10
Q

what does the atomic number contain

A

proton

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11
Q

calculation for relative atomic mass

A 
sum of(isotope abundance*isotope mass number)/
sum of abundance of all isotopes
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12
Q

what are compounds

A

substances formed from two or more elements and are held together by chemical bonds

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13
Q

what is making bonds

A

involves atoms giving away, taking or sharing electrons

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14
Q

how a compound made from a metal and non metal works

A

the metal atoms lose electrons to form positive ions and the non metal gains electrons to form negative ions. This is called ionic bonding because the opposite ions are attracted to each other.

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15
Q

how a compound made from two non metals work

A

consist of molecules, each atom shares an electron with another atom. This is called convalent bonding

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16
Q

what are the properties of a compound compared to the original elements

A

totally different

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17
Q

What are mixtures

A

no chemical bond between the different parts of a mixture and can be separated by physical methods.

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18
Q

Examples of mixtures

A

Air, Crude oil

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19
Q

what are the properties of a mixture compared to the original elements

A

they are a mixture of each part

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20
Q

How were elements arranged in the 1800

A

scientists had no idea of the atomic structure and could only measure relative atomic mass and so elements were in order of atomic mass.

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21
Q

How did Dmitri mendeleev change the periodic table. 1869

A

he made the periodic table in order of atomic mass but swapped them if the properties were similar. He left gaps in the table to make sure elements with similar properties stayed in the same groups and some were undiscovered elements. The elements were discovered and supported his theory.

22
Q

how are elements with similar properties layed out on the periodic table

A

in columns

23
Q

what does the group of the periodic table say

A

it tells you how many electrons are in the outer shell except for group 0

24
Q

why do metals find it easy to form positive ions

A

metals to the left don’t have many electrons and metals at the bottom have electrons far away fro the nucleus meaning not much energy is needed to remove electrons making them form positive ions.

25
Q

why do non metals find it easier to form negative ions

A

they have lots of electrons to remove or the outer electrons are close to the center meaning they have a strong connection. Which means it is easier to gain electrons to form negative ions

26
Q

physical properties of metals

A

strong, malleable, high melting and boiling points, conducting heat and electricity, ductile

27
Q

physical properties of non metals

A

dull looking, brittle low density, not good at conducting

28
Q

special properties of transition metals

A

can have more than one ion
ions are often colored
make good catalysts

29
Q

why are alkali metals so reactive

A

only contain one electron it the outer shell

30
Q

properties of alkali

A

soft, low density, reactive

31
Q

what happens as you go down the alkali column

A 
increasing reactivity(electron is further away from center)
lower melting and boiling points
higher relative atomic mass
32
Q

what kind of ion and bond does an alkali have

A

+1 ions and have ionic bonding

33
Q

equation of alkali with water =

A

alkali hydroxide + hydrogen

34
Q

equation of alkali with chlorine =

A

alkali chloride

35
Q

reaction with oxygen alkali

A

form metal oxides

36
Q

how are alkalis different to transition metals

A

more reactive
less dense, string and hard
lower boiling points

37
Q

colour of Flourine gas

A

yellow/poisonous

38
Q

colour of chlorine gas

A

dense green/poisonous

39
Q

colour of bromine gas

A

red-brown/poisonous

40
Q

colour of iodine

A

purple vapour or dark gray solid/poisonous

41
Q

what happens as you go down the halogen group

A

less reactive
higher melting and boiling points
higher relative atomic masses

42
Q

covalent bonding of halogens

A

share electrons with other non metals and when they react have simple molecular structures

43
Q

ionic bounds of halogens

A

from 1- ions called halides when they bond with metals.

the compounds that form are ionic structures

44
Q

what happens when more reactive halogens react with less reactive ones

A

the more reactive one displaces the less reactive and the salt

45
Q

what happens when chlorine reacts with bromine

A

bromine is kicked from the solution

46
Q

what is group 0

A

noble gases

47
Q

why are noble gases unreactive

A

they have eight electrons making there outer shell full, making them inert

48
Q

what does inert mean

A

unreactive

49
Q

properties of noble gases

A

colorless at room temp

non flammable

50
Q

what happends as you move down the noble gas group

A

boiling points increase

51
Q

why do noble gases increase in boiling point

A

an increase in the number of electrons in each atom leading to greater intermolecular forces between each one

Sciene Chem (14 decks)

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