Unit 1 Flashcards

1
Q

Particle theory of matter

A

John Dalton

1) All matter is made up of particles
2) Atoms can’t be broken down further
3) Atoms can be rearranged with each other
4) Atoms of the same element are the same

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2
Q

Valance shell

A

Outermost shell, only electrons that can change

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3
Q

Atomic number

A

Number of protons and electrons

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4
Q

Atomic mass

A

Total mass of protons and neutrons. Atomic mass- atomic number = number of neutrons

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5
Q

Octet rule

A

Atom is most stable with a full shell of electrons

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6
Q

Ions

A

Atoms that become charged through chemical bond s

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7
Q

Anion

A

Negative, gains electrons. Non metals

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8
Q

Cations

A

Positive, looses electrons. Metals

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9
Q

Isotopes

A

A form of an element where the number of protons stays the same but the number of neutrons changes

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10
Q

Isotopic abundance

A

What % of an isotope exists. Average atomic mass= (iso1)x+ (iso2)(1-x)

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11
Q

Periodic law

A

If they are in the same column, they react the same because they have the same number of valence electrons. The further down you go, the more reactive you get

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12
Q

Necular strength

A

The more protons, the greater the charge and make the atomic radio smaller because they draw electrons in

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13
Q

Ionization energy

A

The amount of energy required to pull electrons away from an element

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14
Q

Electron affinity

A

Energy change when a neutral atom gains an electron

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15
Q

Electronegativity differences

A

The amount of energy required to pull electrons away from other atoms

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16
Q

Ionic electronegativity difference

A

Greater then 1.7

17
Q

Polar covalent

A

1.7-0.5

18
Q

Covalent (non polar)

A

Below 0.5

19
Q

Radioactive decay

A

When unstable isotopes all of a sudden disintegrate

20
Q

Most common types of necular radiation

A

Alpha particles- Positively charged. Same structure of the nucleus of a helium atom. Slow moving
Beta particle- Negatively charged, identical to an electron. Fast moving
Gamma ray- High energy, electromagnetic. Fast moving

21
Q

When a molecule is polar it has….

A

Unequal sharing of electrons

22
Q

When a molecule is not polar is has…

A

Equal sharing of electrons

23
Q

Diatomic gasses

A

Hydrogen, oxygen, nitrogen and column 17

24
Q

Intermolecular forces

A

Weak attractions between particles, not even 1/100 as strong as a bond

25
Q

Vander walls forces

A

Hydrogen bonding >dipole dipole> londen dispersion force

26
Q

Hydrogen bonding

A

H atoms are attracted to highly electronegative atoms (NOF)

27
Q

Dipole dipole forces

A

Attraction between the partial positive and negative charges of polar molecules

28
Q

Londen forces

A

The electrons in one molecule are attracted to the protons in another molecule. They are typically exhibited in non polar molecules. Happens because of temporary un balance of electrons. The more electrons, the greater the charge

29
Q

John Dalton

A

Billiard Ball model

30
Q

J.J. Thompson

A

Plum pudding model, discovered the electron

31
Q

Ernist Rutherford

A

Discovered the nucleas and protons

32
Q

Chadwick

A

Discovered neutrons

33
Q

Neils Bohr

A

Discovered hydrogen has a unique arrangement and that electrons orbit the atom

34
Q

When is ionization energy low

A

When the atomic radius is large therefore the electron s are far away from the nucleus (atomic radius increases with ionization energy and electron affinity)