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chemistry gcse > topic 1 - key concepts in chemistry > Flashcards

topic 1 - key concepts in chemistry Flashcards

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1
Q

describe the history of the atom

A

dalton - atoms as solid spheres with different spheres making up different elements
jj thompson - plum pudding model
rutherford - nuclear model - result from gold foil experiments
bohr model - electrons and shells

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2
Q

what were the 3 key ideas of Daltons model?

A
  1. matter is made of atoms (tiny particles) which cannot be created, destroyed or divided.
  2. atoms of same element are identical
  3. different atoms combine to form new substances
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3
Q

where is the mass of an atom concentrated?

A

nucleus (positively charged)

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3
Q

what are the 3 subatomic particles?

A

protons, neutrons, electrons

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3
Q

what holds an atom together?

A

electrostatic force of attraction between positive nucleus and electrons

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4
Q

what is the charge of a proton?

A

+1

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5
Q

what is the relative mass of a proton?

A

1

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6
Q

what is the charge of a neutron?

A

0 (neutral)

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6
Q

what is the relative mass of a neutron?

A

1

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7
Q

what is the charge of an electron?

A

-1

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7
Q

what is the relative mass of an electron?

A

1/1840

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8
Q

how small is the nucleus’ radius?

A

10 000 x smaller than the atom

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9
Q

define mass number (atomic mass)

A

sum of protons and neutrons in nucleus of an atom

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9
Q

define the atomic number

A

number of protons in the nucleus of the atom

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9
Q

define an isotape

A

an atom with the same number of protons but different number of neutrons

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10
Q

what does the atomic number equal?

A

number of protons

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11
Q

how do you find the number of neutrons?

A

mass number - number of protons

12
Q

how do you find the number of electrons?

A

atom = neutral + has the same number of protons and electrons

13
Q

RAM calculation formula

A

(% of isotope a x mass of isotope a) + (% of isotope b x mass of isotope b) / 100

14
Q

how did Mendeleev organise his periodic table?

A

by mass, and columns contained elements with similar properties

15
Q

why did Mendeleev leave gaps in the periodic table?

A

for elements he believed to be undiscovered and keep elements with similar properties in the same vertical groups.

16
Q

what were the problems with the mendeleevs table?

A

-isotapes were not known and he made no room for them
-discovery of the proton leading to atomic number was not discovered

17
Q

how are elements arranged in the modern periodic table?

A

increasing atomic number

18
Q

what are groups for?

A

vertical columns - show how many outer electrons each atom has

19
Q

what are the periods for?

A

horizontal row - show number of shells of electrons an atom has

20
Q

what happens when you go down the group?

A

outer shell of electrons become further away from nucleus
-weakens their attraction

21
Q

describe ionic bonding

A

an electrostatic force of attraction between oppositely charged ions between a non-metal and a metal

22
Q

what is a cation?

A

a positively charged ion

23
Q

what is an anion?

A

negatively charged ion

24
Q

what are the charges holding the lattice together in ionic bonding?

A

strong electrostatic forces of attraction

25
Q

what is an ionic lattice?

A

a repeating pattern of positive and negative ions

26
Q

do ionic substances have a low of high melting point and boiling point?

A

high

27
Q
A
28
Q

which groups ions have electronic structure of a noble gas?

A

1,2,6, and 7

29
Q

what endings are used for negatively charged ions of a compound?

A

-ide = contains 2 elements (1 is non-metal)
-ate = contains at least 3 elements (one is oxygen)

30
Q

what does oxide involve?

A

O2- ion

31
Q

what does hydroxide involve?

A

OH-

32
Q

what does halide ion involve?

A

-1 halide ion

33
Q

what does nitrate involve?

A

NO3-

34
Q

what does carbonate involve?

A

CO32-

35
Q

what does sulfate involve?

A

SO42-

36
Q
A

chemistry gcse (9 decks)

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