Atoms, Molecules, bonding, Ions Flashcards

1
Q

Matter is

A

Anything that takes up space and has mass

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2
Q

A substance

A

A form of matter that has a definite composition

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3
Q

A mixture

A

A combination of two or more substances

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4
Q

Homogeneous mixture

A

A mixture which is uniform throughout

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5
Q

Heterogeneous mixture

A

A mixture which does not have the same composition throughout

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6
Q

An element

A

A substance which cannot be seperated into simpler substances

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7
Q

A compound, molecule or chemical

A

A combination of two or more different elements. Chemical, or molecule

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8
Q

Physical change

A

A change that does not alter the composition of a compound or element. Ice melting, water evaporating.

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9
Q

Chemical change

A

Altering of the composition of the substances involved.

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10
Q

Extensive property of a material

A

Dependent upon the amount of the substance present.

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11
Q

0 degrees Celsius = K?

100 degrees Celsius = k?

A

0 degrees C = 273 Kelvin

100 degrees C = 373 kelvin

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12
Q

Density equation?

A

Density = mass/volume

1g/cm3 =1g/mL

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13
Q

How many significant digits in 0.08

A

Only 1 significance

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14
Q

Addition and subtraction significant figures

A

The answer cannot have more digits to the right of the decimal than any of the original numbers.

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15
Q

Multiplication and devision, sig figs

A

The number of the significant figures is set by the original number that has the smallest number of significant figures.
Eg. 6.8/112.04 = 0.0606926 = 0.061

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16
Q

Exact numbers

A

Always exactly the number, no decimals or rounding. No need to follow significant figure rules.

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17
Q

Compound is

A

Atoms of more than one element

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18
Q

Chemical reactions

A

Rearrangement of elements and atoms to create a new compound

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19
Q

What is a cathode ray tube?

A

Instrument to measure mass/charge of e-

Jj Thompson Nobel prize winner

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20
Q

Atomic number

A

Number of protons in the nucleus

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21
Q

Mass number

A

Number of protons + number of neutrons

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22
Q

Isotopes

A

Atoms of the same element with different numbers of neutrons in their nuclei.

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23
Q

Empirical formula

A

Shows the simplest whole-number ratio of the atoms in a substance

24
Q

Ionic compounds

A

Consist of a combination of cations and anions

25
Q

Cation position

A

Always on the left,

Anion always positioned to the right.

26
Q

Ionic compounds

A

Often a metal + a non metal

Anion (non metal) add ide to element name.

27
Q

Nomenclature; metal ionic compounds, indicate charge with Roman numerals.
What is FeCL2
Use chemical table.

A

Iron (ii) chloride

28
Q

The prefix; Tetra?

A

4

29
Q

The prefix;

Penta

A

5

30
Q

The prefix;

Henta

A

7

31
Q

The Prefix;

Nona

A

9

32
Q

When to use a prefix

A

If more than one compound can be formed from the same elements prefixes must be used.

33
Q

Name N2Cl4

A

Dinitrogen tetrachloride

34
Q

Anion possible charges

A

Only one possible charge

35
Q

The 5 Cations with more than 1 possible charge;

A

Iron, copper, chromium, manganese, cobalt,

36
Q

What is an acid

A

Is a substance that yields hydrogen ions H+ when dissolved in water.

37
Q

What is a base

A

A substance that yields hydroxide ions OH- when dissolved in water.

38
Q

The 6 Noble gases

A

He, Ne, Ar, Kr, Xe, Rn

39
Q

The 4 most common Halogens;

A

F, Cl, Br, I

40
Q

What is a subscript?

A

The 2 in H2O ect.

41
Q

What is a coefficient in chemistry?

A

The 2 in (2O3)

42
Q

Hydrogen bonding

A

Only with N,O or F.
Dipole-dipole interaction on steroids.
Weak bond, although stronger than dipole-dipole and intermolecular forces.

43
Q

Adhesion

A

Capillary action where water molecules are attracted to the side of the capillary, climbing up.

44
Q

Cohesion

A

Intermolecular attraction to like like molecules.

45
Q

Octet rule

A

Atoms except H tend to form bonds until they are surrounded by 8 electrons.

46
Q

Valence electrons

A

Amount of electrons in an atoms outer most ring.

47
Q

Metallic bonds

A

Delocalisation of electrons.

48
Q

Covalent bond

A

Equal sharing of electrons.

49
Q

Double covalent bond

A

Sharing of 2 electrons in each atom = a total of 4 electrons shared.

50
Q

Triple covalent bond

A

Each atom shares three electrons with an adjacent atom that also shares three electrons = total of 6 electrons shared.

51
Q

Covalent bond electronegativity difference

A

0-0.3

52
Q

Polar covalent bond electronegativity difference

A

0.5-1.6

53
Q

Ionic bond electronegativity difference

A

> 2

54
Q

Resonance structure

A

1 of 2 or more Lewis structures for the same molecule.

55
Q

Look for lone pair when drawing Lewis structures, this changes shape of molecule encouraging it to be polar.

A

Shared covalent bonds create non linear molecular shape.

56
Q

Spectator ions

A

Are ions which do not change states in a chemical reaction. (l,s,g).