Ch. 3 Atoms

Atoms of the same element that have different masses due to different numbers of neutrons.

The amount of substance that contains as many particles as there are atoms in 12 g of carbon-12

The very small, very dense center part of an atom. 

The atomic number (Z) represents the number of these in an atom.

This law holds that compounds of the same elements combine in simple whole number ratios.

Proposed the plum pudding model of chemistry.

The nucleus of an atom consists of these 2 kinds of subatomic particles.

The force that holds protons and neutrons together in the nucleus.

The number of these determine an atom’s identity as an element.

This part of an atom has approximately 1/2000^th the mass of a hydrogen atom.

English schoolteacher who proposed atomic theory to explain newly discovered laws. 

Scientist who performed the gold foil experiment. 

Ancient Greek thinker who proposed that all matter is made of atoms.

The "father of chemistry," his work led to the discovery of the law of conservation of mass.

This law holds that a compound contains the same proportions by mass regardless of sample size.

The units used in molar mass.

Dalton incorporated the law of conservation of mass into his theory by asserting that atoms are

The charge of the particles that make up the cathode ray in the cathode-ray experiments.

The number of atoms in 1 mol of a substance.

The mass in grams of 2.0 moles of oxygen (if the molar mass of O = 16 grams/mol)

The mass of one mol of a substance is called this

This law holds that matter is neither created nor destroyed during chemical reactions.

This part of the atom consists of mostly empty space.

The positively charged electrode of a cathode-ray tube is called this.