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Chemistry > C1 > Flashcards

C1 Flashcards

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1
Q

definition of ion

A

Ion = an atom that has gained a charge by gaining or losing electron(s)

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2
Q

where are metals on the periodic table

A

on the left

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3
Q

where are non-metals found on the periodic table

A

on the right

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4
Q

what are metalloids

A

Metalloids = elements with both metal AND non-metal properties

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5
Q

where are metalloids found

A

The staircase division on the right side shows you where the metalloids are found

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6
Q

what does group number show

A

Group Number = number of outer electrons

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7
Q

what does the period number show

A

Period Number = the number of shells in our atom

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8
Q

what is the relative atomic mass

A

relative atomic mass = the average of the mass numbers of ALL the isotopes of an element, relative to Carbon-12.

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9
Q

definition of isotopes

A

Isotopes = different forms of the same element, with the SAME number of electrons and protons, but DIFFERENT number of neutrons

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10
Q

what does the mass number show

A

number of protons and electrons

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11
Q

what does the atomic number show

A

number of protons or electrons

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12
Q

differences between compound and mixtures (3 each)

A

compounds-
-chemically combined
-seperated using chemical reactions
-have a fixed ratio

Mixtures
-not chemically bonded
-seperated using seperating techniques
-dont have a fixed ratio

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13
Q

what does aqueous mean

A

aqeuous = dissolved in water (looks like aqua which means water)

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14
Q

what is the law of conservation of mass

A

Law of conservation of mass = mass cannot be created or destroyed. –> total mass of the reactants = total mass of the products

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15
Q

define filteration

A

Filtration = a technique that separates the insoluble substances in a solution from the solvent/ any soluble substances

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16
Q

define soluble

A

Soluble = ability to dissolve

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17
Q

define solvent

A

Solvent = a liquid that can dissolve things in it - examples: water, alcohol

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18
Q

define solution

A

Solution = a solute that is dissolved in a solvent

19
Q

whatt is the process of crystallisation

A

Crystallisation is used to separate a solute from a solvent - more specifically the term crystallisation is used when a pure salt is obtained from the salt solution

20
Q

what is the setup for crystallisation

A

In crystallisation here is the set up:
A heatproof mat is placed down. On top of this, a tripod is set up with a wire gauze on top, with the metal crucible dish balanced on this gauze. The bunsen burner is placed underneath the tripod. You slowly evaporate the solvent off. Once it looks mostly gone, you tip out the crystals (you may need to scrape them off the dish) onto a paper towel and leave it in a cool dark place to dry for a few days.

21
Q

breifly describe the set up for distillisation

A

A bunsen burner is placed under the round bottom flask. The liquid with the lower boiling point starts to become a gas first. Whilst this is becoming a gas, the temperature of the mixture does not change. When it comes a gas, it rises and enters the tube sealed within the bung. Through the tube it enters the condensing chamber, which has constantly flowing cold water running around the tube, which makes this gas condense and flow down to be collected into a beaker.

21
Q

define condenser in terms of distillation

A

A condenser = a glass tube with cold water flowing around it

22
Q

define miscible liquids

A

Miscible liquids = liquids that can dissolve in each other mixing completely, like milk and water

22
Q

what happens to things with higher boiling points in a fractionating column

A

Things with higher boiling point condense on the cool beads near the bottom and drips back into the flask

22
Q

define immiscible liquids

A

Immiscible liquids = liquids that can’t dissolve in each other like water and oil

23
Q

what is a fractionating column

A

A laboratory fractionating column is a piece of glassware used to separate vaporized mixtures of liquid compounds with close volatility. Most commonly used is either a Vigreux column or a straight column packed with glass beads

24
Q

what is paper chromatogaphy used for

A

Paper chromatography is used to separate dyes.

25
Q

what does paper chromatography depend on

A

Paper chromatography uses the different solubility of these dyes to do this.

26
Q

define solubility

A

Solubility = the ability of something to dissolve

27
Q

what does solubility in chromatography determine

A

The solubility of the dye/ink determines how far that dye travels with the water up the paper

27
Q

how must the paper be dipped into the water

A

The paper must be dipped below the pencil line so that the ink spot does not dissolve into the solvent pool.

28
Q

what did john Dalton discover about the atom

A

John Dalton - said substances were made out of tiny hard spheres - each chemical element had its own atoms which differed in mass, and these were the fundamental building blocks of nature

29
Q

what had JJ Thompson discovered?

A

JJ Thompson (1800s)- discovered the electron
Thompson came up with the plum pudding model (plum pudding is basically a raisin cake). Plums were electrons, in a ball of positive charge (the pudding).

30
Q

how was the nucleus discovered

A

The nucleus was discovered in the gold foil experiment
Niels Bohr came up with with the modern nuclear model and said electrons must be orbitting the nucleus (modern nucleus = nucleus in middle with circles around it)

31
Q

what did James Chadwick discover

A

James Chadwick discovered the neutrons to explain the missing mass

32
Q

wha did the result of the gold foil experiment prove

A

The results of the gold foil experiment told Rutherford Geiger and Marsden that:
1)Most of the atom is empty –> most of the alpha particles went straight through
2)The nucleus is a positive charge at the centre of the atom –> some of the alpha particles partially refracted
3)The nucleus is very dense and small in the middle of the atom –> a small number of alpha particles refracted completely

33
Q

what are sub-atomic particles

A

Sub-atomic particles = electrons protons and neutrons

34
Q

what are the masses of protons,electrons and nuetrons

A

Masses of:
electron: negligible - 1/1840
Proton: 1
Neutron: 1

35
Q

what are the charges of the sub atomic particle

A

Charges of:
electron: -1
proton: +1 (p for positive)
neutron: 0 (NEUTRon for NEUTRal)
SO the overall charge of the nucleus is positive

36
Q

what is the charge of an atom

A

An atom has a neutral overall charge. All atoms have an equal number of protons and electrons. This means that the total positive charge and the total negative charge is equal, so they cancel each other out, leaving an overall atomic charge of 0.

37
Q

in the periodic table what is the top number and what does it mean

A

In the periodic table, the top number is the relative atomic mass. Relative atomic mass = the average mass of all the isotopes for that element, relative to the mass of Carbon-12

38
Q

what does group number and period number show

A

Group number = the number of outer electrons
Period number = the number of shells

39
Q

what are chemical properties of an atom determined by

A

Chemical properties are determined by the number of outer electrons

40
Q
A

Chemistry (4 decks)

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