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Chemistry > 1&2) Key Concepts in Chemistry A > Flashcards

1&2) Key Concepts in Chemistry A Flashcards

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1
Q

how has the Dalton method changed over time?

A

-discovery of subatomic particles…. electrons

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2
Q

what is the structure of an atom?

A
  • nucleus with protons+neutrons

- electrons surrounding in electron shells

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3
Q

what is the relative mass and relative charge of a proton?

A
  • RC- +1(positive)

- RM- 1

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4
Q

what is the relative mass and relative charge of a neutron?

A
  • RC-0(no charge)

- RM- 1

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5
Q

what is the relative mass and relative charge electron?

A
  • RC- -1(negative)

- RM- 1/1835 (negligible

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6
Q

why do atoms contain equal numbers of electrons and protons?

A
  • no overall charge

- charges cancel out

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7
Q

how big is the atoms nucleus compared to the whole thing?

A

-nucleus can be 100,000 smaller diameter

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8
Q

where is most of the mass in an atom?

A

-in the nucleus

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9
Q

what is the mass number of an atom? where is it found?

A
  • protons+neutrons

- top number

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10
Q

what is the atomic number?where is it found?

A
  • protons only

- bottom number

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11
Q

what is an isotope?

A
  • same element
  • same atomic number
  • different mass number
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12
Q

if you have the mass number and atomic number how do you work out how many protons, neutrons and electrons there are?

A

atomic number= -number of protons
-same number of electrons
mass number= neutrons+protons

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13
Q

what are relative atomic masses compared to?

A

-carbon-12

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14
Q

how does the existence of isotope result in not having whole number relative atomic masses?

A
  • takes into account all of the isotopes

- amount of each isotope

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15
Q

how do you work out the relative atomic mass?

and what is the symbol for RAM?

A

number of atoms
-Ar

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16
Q

EXAMPLE
if the abundances of the two isotopes of chlorine are 75% of 35. and 25% of 37
CL CL.
17 17
how do you work out the relative atomic mass?

A 
         100
17
Q

how did Mendeleev arrange the elements known at the time?

A
  • order of RAM (but he wasn’t always right)
  • left gaps
  • swapped them to suit their chemical properties and their compounds
18
Q

how did Mendeleev use the table to predict elements not discovered?

A

-properties of near by elements

19
Q

how are elements arranged in the periodic table today?

A
  • elements in rows/periods are increasing atomic number order
  • smilar properties in the same colour/group
  • non metals ont he right
20
Q

what are the connections with the electric configuration and the periodic table?

A
  • number of shells is equal to period number

- number of electrons in the outer shall is the same to the group number

21
Q

how are cations formed?

A
  • metal atoms
  • loose electrons
  • form positive ions
22
Q

how are anions formed?

A
  • non metals
  • gain electrons
  • form negative ions
23
Q

what is an ion?

A

-an atom or group of atoms with a positive or negative charge

24
Q

in group 1 how many outer electrons are there? how many electrons lost or gains? charge on ion? example.

A
  • 1 electron in the outside shell
  • 1 electron lost
  • 1+ charge
  • Li+
25
Q

in group 2 how many outer electrons are there? how many electrons lost or gains? charge on ion? example.

A
  • 2 electrons in the outside shell
  • 2 electrons lost
  • 2+ charge
  • Ca^2+
26
Q

in group 6 how many outer electrons are there? how many electrons lost or gains? charge on ion? example.

A
  • 6 electrons in the outer shell
  • 2 electron gained
  • 2- charge
  • S^2-
27
Q

in group 7 how many outer electrons are there? how many electrons lost or gains? charge on ion? example.

A
  • 7 electrons in the outer shell
  • 1 electron gained
  • 1- charge
  • F-
28
Q

what does it means when a compound ends in -ate or -ide?

A

-ion contains oxygen

29
Q

Examples of ionic compounds coming together:

sodium sulfide contains the ions Na+ and S2-

A

-Na˘2S

30
Q

what is the structure of an ionic compound?

A
  • strong electrostatic forces

- arranged in lattice structure

Chemistry (11 decks)

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