Chap 3 Flashcards

1
Q

The four key features of Dalton’s atomic theory

A
  • Elements are made of tiny, indivisible particles called atoms
  • Atoms combine/can join together in whole number ratios (to form compounds).
  • Atoms of each element are unique
  • Atoms are unchanged in chemical reactions.
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2
Q

The atom is

A

The fundamental unit of matter.
Each element is composed of a different type of atom, which gives each element its unique properties.
(‘atom’ derived from ‘atomos’, meaning: “indivisible”)

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3
Q

The Law of Conservation of Mass (Antoine Lavoisier, born 1794)

A

States: “In chemical reactions, matter is neither created nor destroyed”

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4
Q

The three foundational ideas:

A
  • All mater is composed of atoms
  • The atoms of each element have unique characteristics and properties
  • -In chemical reactions. atoms are not changed, but combine in whole number ratios to form compounds.
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5
Q

Can we see atoms?

A

No. Atoms are too small to be seen with a naked eye, or even a microscope.
Scientists use x-ray crystallography to visualize the arrangement of atoms.

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6
Q

The Periodic table arrangement

A

Rows(horizontal)- called “periods”

Columns(vertical)- called “groups” or “families”

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7
Q

Main group elements locations

A

The two side blocks (Columns 1A-2A (1&2) and 3A-8A(13-18))

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8
Q

Location of the transition & inner transition elements

A

Block between the main group elements blocks (columns 3-12)

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9
Q

Subatomic particles

A

Particles that make up atoms

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10
Q

Location of Alkali Metals

A

Collum 1A

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11
Q

Location of Alkaline earth metals

A

Collum 2A

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12
Q

Location of Halogens

A

Collum 7A

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13
Q

Location of Noble Gasses

A

Collum 8A

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14
Q

Mass number =

A

protons + neutrons

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15
Q

Atomic Theory

A

a theory describing matter in terms of fundamental units, atoms

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16
Q

Atomic mass unit (u or amu)

A

A unit of mass equal to 1.66x10^-27kg

17
Q

Charge

A

a characteristic property of subatomic particles that affects how particles interact with each other

18
Q

Electron

A

A negatively charged sub-atomic particle. the electrons occupy the space around the nucleus.

19
Q

Nucleus

A

The tiny, dense center of an atom. The nucleus contains protons and neutrons.

20
Q

Electron cloud

A

the space around the nucleus. Accounts for nearly the entire volume of the atom

21
Q

Atomic number

A

The number of protons in an atom, also the number of electrons in a neutral atom

22
Q

What are six evens in uncovering atomic structure?

A

1) Volta’s electrochemical cell
2) Dalton’s atomic theory
3) Mendeleev’s periodic table
4) Thomson discovers the electron
5) Plum pudding model
6) Rutherford proposes the nucleus

23
Q

Isotopes

A

Atoms that have the same atomic number but different mass numbers

24
Q

Plum pudding model

A

Negative electrons spread throughout a positive material

25
Q

Net charge(total charge/ overall charge?)

A

= #Protons - #electrons

26
Q

Bohr model

A

Electrons orbit the nucleus like planets orbit the sun

27
Q

Quantam model

A

Electrons behave both as particles and waves

28
Q

Atoms gain or loose electrons to form

A

Ions

29
Q

Ion

A

atom or group of atoms with an overall charge

30
Q

average atomic mass

A

weighted average of the different isotopes of an element